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1. A. B. C. D. * E. 2. A. B. * C. D. E. 3. A. B. C. D. * E. 4. A. B. C. D. E. * 5. A. B. C. D. E. * 6. A. * B. C. D. E. 7. A. B. * C. D. E. What’s following process that has ∆S0›0? All correct NH4NO2(s) → 2Н2О(g) + N2(g) no one 2H2S(g) + 3O2(g) → 2Н2О(g) + 2SO2(g) 2СО(g) + О2(g) →2СО2(g) Where will the process be spontaneous? Q=0, ∆S0›0 ∆Н0‹0, ∆S0›0 no one ∆Н0›0, Т=0 ∆Н0›0, ∆S0‹0 For what is substance the standard enthalpies of formation equal 0? NO HF(l) Н2О(g) N2(g) HF(g) For what is substance the standard enthalpies of formation equal 0? NO С6Н12О6 Н2O СО2 О2 How will the rate of reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if pressure will increase on 3 times in the system? increase on 9 times decrease on 3 times increase on 3 times decrease on 27 times increase on 27 times How will the rate of this reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if a pressure will decrease on 2 times in the system? decrease on 8 times decrease on 2 times increase on 2 times increase on 6 times increase on 8 times The temperature coefficient = 3. How much will the rate of reaction increase at the increasing temperature on 20 0C? on 8 times on 9 times on 3 times on 20 times on 2 times 8. A. B. C. D. E. * 9. A. * B. C. D. E. 10. A. B. C. * How will the rate of this reaction 2 Cl2O = 2 Cl2 + O2 will change if the concentration of Cl2O will increase on 3 times? increase on 6 times decrease on 3 times increase on 3 times decrease on 9 times increase on 9 times How will a rate of a simple chemical reaction change 2A → B + C at an increasing of initial concentration on 2 times? increase on 4 decrease on 4 increase on 2 will not change decrease on 2 Dependence the rate constant from the temperature is determination according to: k1 k0 1 1 ln c0 c c0 c k Ae Ea RT 1 c0 с c0 с D. k E. 1 2 11. A. For this equation 2Fe(s) + 3Cl2 = 2FeCl3 the rate law is: 1 k с0 CCl3 2 B. k C 2Fe CCl C. k C Fe C3Cl 2 D. k C 2Fe C3Cl E. * 12. A. k C3Cl 2 2 2 For this equation С(s) + О2 = СО2 the rate law is: CO2 CC 2 B. 2 k CO CC 2 C. k CO 2 C C D. 2 k CO 2 2 k CO 2 E. * k CO 2 13. Record of reaction of N2(g)+ O2(g.)= 2NO(g.) - 180,8 kJ/mol means that: A. B. C. D. * E. 14. A. B. * C. D. E. 15. A. B. C. * D. E. 16. A. B. C. D. E. * 17. A. B. C. * D. E. 18. A. B. C. * D. E. 19. A. B. * C. D. E. 20. A. For formation 2 mol NO is selected 90,4 kJ heat For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat Under formation of 1 mol of NO 90,4 kJ heat is released For formation 1 mol of NO is taken of 180,8 kJ heat To determine, without any calculation, what is the following process that is true of the oxidation reaction of Glucose: С6H12O6 (l)+ 6O2(g)= CO2(g) + 6H2O(l), H = -2803kJ Q 0, S 0 H 0, S 0 H 0, S 0 H 0, S 0 H 0, S 0 How much will temperature increase that the rate will increase on 64 times if temperature coefficient = 2? 40 0C 80 0C 60 0C 50 0C 70 0C Temperature coefficient shows how much… The equilibrium constant increases on 10 0C at increasing temperature The rate’s constant increases on 1 0C at increasing temperature The rate’s constant increases on 10 0C at increasing temperature The rate of chemical reaction increases on 1 0C at increasing temperature The rate of chemical reaction increases after at temperature increas on 10 0 C From what factors doesn’t depend the rate constant of the chemical reaction? The nature of reactants The catalyst presents The concentrations of reactants The concentrations of reactants and pressure Temperature and time The rate of the chemical reaction is: All are right The quantity change of the number of reactants according to the specific time The concentration change of a reactant according to the specific time The temperature change of a reactant according to the specific time The volume change of a reactant according to the specific time What are the molecularity and the order of a forward reaction 2НІ = Н2+ І2: Termolecular the first order Bimolecular the second order Bimolecular the first order Unimolecular the second order Unimolecular the first order The values of Molecularity and the order as a rule are: 2-3, 2-3 corresponding B. C. D. E. * 21. A. B. C. D. E. * 22. A. B. * C. D. E. 23. A. B. C. D. E. * 24. A. B. C. D. * E. 25. A. 2-3, 1-3 corresponding 0-3, 0-3 corresponding 1-3, 1-3 corresponding 1-3, 0-3 corresponding For what kind of process using Gibbs’ free energy? Isobaric Isochoric Adiabatic Isothermic-isochoric Isothermic-isobaric What can you define using ΔG? Chemical rate Direction of chemistry reaction Volume Temperature Pressure What kind of properties has the entropy? Extensive and Intensive Intensive A state function Intensive and state function Extensive and a state function What kind of change is indentified the entropy? Irreversable No one Permissible changes & Spontaneous changes Spontaneous changes Reversable changes What is find the entropy change? B. C. * D. ^ S = sum Sproducts = sum Sreactants ΔS = sum Sproducts – sum Sreactants ΔS = 1 – (sum Sproducts + sum Sreactants) E. Δ S = sum Sreactants + sum Sproducts Δ S = sum Sreactants – sum Sproducts 26. A. B. * C. D. E. 27. A. Formula of Entropy are: S = U+W S = Q/T S = U-W S = T/Q S = U + dΔV What is sign of the enthalpy for endothermic process? -ΔS0 B. +ΔS0 -ΔH0 0ΔH0 C. D. E. * 28. A. B. C. D. E. * 29. A. B. C. D. * E. 30. A. B. C. D. E. * 31. A. B. C. D. E. * 32. A. B. C. D. E. * 33. A. B. C. D. E. * 34. A. B. * +ΔH0 How is calculate the enthalpies of reactions? All correct ΔH0 = ( Sum of the standard enthalpies of formation of products) : ( Sum of the standard enthalpies of formation of reactants) ΔH0 = (Sum of the standard enthalpies of formation of reactants) - ( Sum of the standard enthalpies of formation of products) ΔH0 = ( Sum of the standard enthalpies of formation of products) + ( Sum of the standard enthalpies of formation of reactants) ΔH0 = ( Sum of the standard enthalpies of formation of products)-( Sum of the standard enthalpies of formation of reactants) Record of reaction of N2(g)+ O2(g.)= 2NO(g.) – 180,8 kJ/mol means that: For formation 2 mol NO is selected 90,4 kJ heat For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat For formation 1 mol NO is released 90,4 kJ heat For formation 1 mol of NO is taken of 180,8 kJ heat What is the law: name energy can neither be created no destroyed although it may be transfered from one form to another? Kirkhgof‘s law Gess’ law A third law of thermodynamics A second law of thermodynamics A first law of thermodynamics In some systems which are used in pharmaceutical technology volume does not changes. What is kind of the correlation among internal energy and enthalpy in such systems? U = 2H 2U = 2H ΔU > ΔH ΔU < ΔH ΔU = ΔH What is the process according to this reaction of H2(g)+ Cl2(g) → 2HCl(g) + Q= -ΔH: Intencive Extensive Adiabatic Endothermic Exothermic Enthalpy is measured in: kkal/K kJ/mol*K kkal kJ kJ/mol What are the intensive properties of the thermodynamics system: Initial energy Concentration C. D. E. 35. A. B. C. * D. E. 36. A. B. * C. D. E. 37. A. B. C. * D. E. 38. A. B. C. D. * E. 39. A. B. C. * D. E. 40. A. B. C. D. * E. 41. A. * B. C. D. E. Internal energy Volume Mass What is the function that doesn’t depend on the passing way of a reaction but depends on the initial and the final state of a system? Volume Pressure Enthalpy Work Heat Process, when there is V constant is ... Isothermal Isochoric Isobaric Isochoric– isothermal Isobaric– isothermal Open thermodynamic systems are exchanged with an environment: By nothing By components By a matter and energy By energy By a matter How can you classify thermodynamics systems according to their phases? Irreversible and reversible equilibrium and unequilibrium Isolated, opened, closed Homogeneous and heterogeneous Solid, liquid, gaseous Standard condition are when the values of pressure and temperature eqwual: 50 kPа, 298 K 50 kPа, 273 K 101,3 kPа, 298 K 101,3 kPа, 273 K 101,3 kPа, 0 K When the pressure and the volume are constant. What is name of this thermodynamic process? Isothermal Isochoric Isobaric Isobaric – isochoric Isochoric– isothermal Calcium is.... bond: Metallic Nonpolar covalent Polar covalent Hydrogen Ionic 42. A. B. C. * D. E. 43. A. B. C. D. E. * 44. A. B. * C. D. E. 45. A. B. C. * D. E. 46. A. B. C. D. * E. 47. A. B. C. D. E. * 48. A. B. C. * D. E. 49. A. B. C. * Hydrogen has ionic bond in compound: C2H2 CH4 CsH HCl H2 Oxygen has nonpolar covalent bond in compound: СО CaO K2O CO2 O2 The greatest electronegativity has element: Li Cl Br P Si All compounds have ionic bond: H2S, K2S SO2, H2SO3 NaCl, KCl Cl2, SO2 HCl, HBr All compounds have nonpolar covalent bond: NaCl, H2O, H2S H2SO4, K2SO4 NaCl, KCl N2, O2, Br2 HCl, HBr, H2O All compounds have polar covalent bond: NaCl, Cl2, H2 H2SO4, K2SO4 NaCl, KCl Cl2, H2, Br2 HCl, HBr, H2O What molecule has multiple bonds? I2 HCl N2 H2 polar molecule The most polar is ….bond: Hydrogen Metallic Ionic D. E. 50. A. B. C. D. E. * 51. A. B. C. D. * E. 52. A. * B. C. D. E. 53. A. B. * C. D. E. 54. A. B. C. * D. E. 55. A. B. C. D. E. * 56. A. B. C. * D. E. 57. A. Nonpolar covalent Polar covalent Intermolecular hydrogen bond is between molecules of: F2 K2S N2 H2 HF Between water molecules are…. bond Metallic Nonpolar covalent Polar covalent Hydrogen Ionic All compounds have polar covalent bond except: O3 NH3 HF H2O H2SO4 What molecule has nonpolar covalent bond? NO H2 HF H2O H2SO4 Choose a compound which has nonpolar covalent bond is: Cu H2S F2 H2O K2O Choose a compound which has ionic bond is: Cu H2S F2 H2O K2O How many periods are in the periodical table of D. Mendeleev? 6 8 7 4 3 The greatest nonmetallic properties has: S B. C. D. * E. 58. A. B. C. D. * E. 59. A. B. C. D. E. * 60. A. B. * C. D. E. 61. A. B. C. D. * E. 62. A. * B. C. D. E. 63. A. * B. C. D. E. 64. A. B. C. D. E. * Na Cl F Ag The greatest metallic properties has: Li Na Cl Fr F How many electrons are at f-lever? 8 10 16 6 14 How many electrons are at d-lever? 8 10 16 6 2 How many electrons are at p-lever? 7 32 16 6 2 How many electrons are at s-orbital? 2 32 16 8 3 The smallest unit of a chemical element that has the properties of that element is called: Atom Molecule Nucleon Electron Neutron What is spin? Type of hybridization Electronic orbitales Charge of nucleus of atom Electronic density Own motion of electron is about axis 65. A. B. C. D. * E. 66. A. B. C. * D. E. 67. A. B. C. * D. E. 68. A. * B. C. D. E. 69. A. B. C. D. * E. 70. A. B. * C. D. E. 71. A. B. C. D. * E. 72. A. B. * Two or more atoms having the same atomic number but differing in atomic weight and mass number is named: Protons Isochors Isotones Isotopes Spin Five electrons on a p electronic level have an atom: Argon Neon Fluorine Nitrogen Carbon The atomic mass is determined as: Sum mass of all electrons which are in atom Sum mass of neutrons which are in nucleus Sum mass of all protons and neutrons which are in nucleus Sum mass of all electrons which are in main electronic levels Sum mass of protons which are in nucleus What particle is influence for charge of atomic nucleus? Amount of protons Amount of electrons Common amount of nucleons Amount of neutrons Amount of positrons What particle is not in the atomic nucleus? Any one Proton Nucleon Electron Neutron Non-salts forming oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Amphoteric oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Complex substances are all except: HCl Cl2 C. D. E. 73. A. B. C. * D. E. 74. A. B. C. D. E. * 75. A. B. C. D. E. * 76. A. B. C. D. * E. 77. A. B. C. * D. E. 78. A. * B. C. D. E. 79. A. * B. C. D. E. 80. Fe(OH)3 MgO BaCO3 Acidic oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Basic oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Salts are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3, CaCl2, MgCl2, Na3PO4,Ca3(PO4)2 Oxides are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Bases are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Acids are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Complex salts are: [Ag(NH3)2]Br, Na[Ag(CN)2] NaHCO3, Na2HPO4 CaOCl2, KAl(SO4)2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Mixed salts are: A. B. C. * D. E. 81. A. B. C. D. E. * 82. A. * B. C. D. E. 83. A. B. * C. D. E. 84. A. B. C. D. * E. 85. A. B. C. * D. E. 86. A. B. * C. D. E. 87. A. * B. C. KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Basic salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Double salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Acidic salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Medium salts are: KAl(SO4)2 NaHCO3, Na2HPO4 Zn(OH)Cl Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Mixed salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical. Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and ions of acid radical Basic salts are: In the time of dissociation gives two cations and one anion Under the dissociation give metal cations, hydroxyl anions and anions of acid Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid In the time of dissociation give only metal cations (or NH4+) and ions of acid Double salts are: Two cations and one anion are created during dissociation In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions D. E. 88. A. B. C. D. * E. 89. A. B. C. D. E. * 90. A. * B. C. D. E. 91. A. B. * C. D. E. 92. A. B. C. * D. E. 93. A. B. C. D. * E. 94. A. B. * In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and ions of acid radical Acidic salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+ ) and ions of acid radical Medium salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and anions of acid radical Salts are: Complex substances, which consist from atoms of metal and acid residuals Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Acids are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting of hydrogen cations and anion Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which is oxygen Compound which molecules consist of one-type atoms Bases are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Oxides are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Monoatomic compound is: Water Helium C. D. E. 95. A. B. C. * D. E. 96. A. B. C. D. E. * 97. A. B. C. D. * E. 98. A. B. C. D. * E. 99. A. * B. C. D. E. 100. A. * B. C. D. E. 101. A. B. C. D. * E. 102. Ozone Ammonia Oxygen Such compound has three atoms in molecule: Aluminum hydride Hydrogen fluorine Hydrogen sulfur Ammonia Methanol Formula of molecule is: ОН3O 2O O-2 O2 Molar mass of sulfuric acid is: 49 g/mole 80 g/mole 106 g/mole 98 g/mole 65 g/mole Mass of three mole of water is: 6g 36 g 48 g 54 g 18 g Relative atomic mass of carbon is: 12 14 6 10 18 Avogadro’s number is: 6.02*1023 6.02*1025 3.01*1023 6.02*1022 3.01*1020 Molar mass of water is: 18 g 17 g/mole 24 g/mole 18 g/mole 16 g/mole Relative atomic mass of Oxygen is: A. B. C. D. E. * 103. A. B. * C. D. E. 104. A. B. C. * D. E. 105. A. B. C. * D. E. 106. A. B. C. D. E. * 107. A. * B. C. D. E. 108. A. B. C. D. E. * 109. A. B. C. * D. 8 15 12 18 16 Molar volume at normal stat (a temperature 273 K and pressure of 101,3 kPa) has: 22,4 m3 22,4 l/mol 11,2 l/mole lest then 22,4 l/mole more than 22,4 l/mole During the physical phenomena: There is a change of quantitative composition of compound There is a change of amount of electrons in an atom There is a change of the aggregate state of compound There is a change only of chemical elements There is a change of qualitative composition of molecules 112 g of nitrogen have volume: 56,9 l 11,2 l 89,6 l 112 l 22,4 l Complex compound: О3 C О2 H2 СО2 Choose correct definition “simple compound is…..” molecules or crystals are contain atoms of one element molecules or crystals are contain atoms of 3th different elements molecules or crystals are contain atoms of one group elements molecules or crystals are contain atoms of 2th elements molecules or crystals are contain atoms of different elements To choose oxygen-containing acids: H2S HBr HCl HI H2SO4 To choose the simple compound: HNО3 CO О2 H2O E. 110. A. B. C. D. * E. 111. A. B. C. D. * E. 112. A. B. C. D. E. * 113. A. B. C. D. E. * 114. A. * B. C. D. E. 115. A. B. * C. D. E. 116. A. B. C. D. СО2 What’s following process that has ΔS0›0? All correct NH4NO2(s) > 2Н2О(g) + N2(g) no one 2H2S(g) + 3O2(g) > 2Н2О(g) + 2SO2(g) 2СО(g) + О2(g) >2СО2(g) For what is substance the standard enthalpies of formation equal 0? NO HF(l) Н2О(g) N2(g) HF(g) For what is substance the standard enthalpies of formation equal 0? NO С6Н12О6 Н2O СО2 О2 How will the rate of reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if pressure will increase on 3 times in the system? increase on 9 times decrease on 3 times increase on 3 times decrease on 27 times increase on 27 times How will the rate of this reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if a pressure will decrease on 2 times in the system? decrease on 8 times decrease on 2 times increase on 2 times increase on 6 times increase on 8 times The temperature coefficient = 3. How much will the rate of reaction increase at the increasing temperature on 20 0C? on 8 times on 9 times on 3 times on 20 times on 2 times How will the rate of this reaction 2 Cl2O = 2 Cl2 + O2 will change if the concentration of Cl2O will increase on 3 times? increase on 6 times decrease on 3 times increase on 3 times decrease on 9 times E. * 117. A. * B. C. D. E. 118. A. B. C. * D. E. 119. A. B. C. D. * E. 120. A. B. C. * D. E. 121. A. B. C. D. E. * 122. A. B. C. D. E. * 123. A. B. C. * D. E. 124. increase on 9 times How will a rate of a simple chemical reaction change 2A > B + C at an increasing of initial concentration on 2 times? increase on 4 decrease on 4 increase on 2 will not change decrease on 2 Dependence the rate constant from the temperature is determination according to: _ _ _ _ _ Record of reaction of N2(g)+ O2(g.)= 2NO(g.) - 180,8 kJ/mol means that: For formation 2 mol NO is selected 90,4 kJ heat For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat Under formation of 1 mol of NO 90,4 kJ heat is released For formation 1 mol of NO is taken of 180,8 kJ heat How much will temperature increase that the rate will increase on 64 times if temperature coefficient = 2? 40 0C 80 0C 60 0C 50 0C 70 0C Temperature coefficient shows how much… The equilibrium constant increases on 10 0C at increasing temperature The rate’s constant increases on 1 0C at increasing temperature The rate’s constant increases on 10 0C at increasing temperature The rate of chemical reaction increases on 1 0C at increasing temperature The rate of chemical reaction increases after at temperature increas on 10 0 C From what factors doesn’t depend the rate constant of the chemical reaction? The nature of reactants The catalyst presents The concentrations of reactants The concentrations of reactants and pressure Temperature and time The rate of the chemical reaction is: All are right The quantity change of the number of reactants according to the specific time The concentration change of a reactant according to the specific time The temperature change of a reactant according to the specific time The volume change of a reactant according to the specific time What are the molecularity and the order of a forward reaction 2НІ = Н2+ І2: A. B. * C. D. E. 125. A. B. C. D. E. * 126. A. B. C. D. E. * 127. A. B. * C. D. E. 128. A. B. C. D. E. * 129. A. B. C. D. * E. 130. A. B. * C. D. E. 131. A. B. Termolecular the first order Bimolecular the second order Bimolecular the first order Unimolecular the second order Unimolecular the first order The values of Molecularity and the order as a rule are: 2-3, 2-3 corresponding 2-3, 1-3 corresponding 0-3, 0-3 corresponding 1-3, 1-3 corresponding 1-3, 0-3 corresponding For what kind of process using Gibbs’ free energy? Isobaric Isochoric Adiabatic Isothermic-isochoric Isothermic-isobaric What can you define using ?G? Chemical rate Direction of chemistry reaction Volume Temperature Pressure What kind of properties has the entropy? Extensive and Intensive Intensive A state function Intensive and state function Extensive and a state function What kind of change is indentified the entropy? Irreversable No one Permissible changes & Spontaneous changes Spontaneous changes Reversable changes Formula of Entropy are: S = U+W S = Q/T S = U-W S = T/Q S = U + d?V How is calculate the enthalpies of reactions? All correct ?H0 = ( Sum of the standard enthalpies of formation of products) : ( Sum of the standard enthalpies of formation of reactants) C. D. E. * 132. A. B. C. D. * E. 133. A. B. C. D. E. * 134. A. B. C. D. E. * 135. A. B. C. D. E. * 136. A. B. * C. D. E. * 137. A. B. * C. D. E. 138. A. ?H0 = (Sum of the standard enthalpies of formation of reactants) - ( Sum of the standard enthalpies of formation of products) ?H0 = ( Sum of the standard enthalpies of formation of products) + ( Sum of the standard enthalpies of formation of reactants) ?H0 = ( Sum of the standard enthalpies of formation of products)-( Sum of the standard enthalpies of formation of reactants) Record of reaction of N2(g)+ O2(g.)= 2NO(g.) – 180,8 kJ/mol means that: For formation 2 mol NO is selected 90,4 kJ heat For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat For formation 1 mol NO is released 90,4 kJ heat For formation 1 mol of NO is taken of 180,8 kJ heat What is the law: name energy can neither be created no destroyed although it may be transfered from one form to another? Kirkhgof‘s law Gess’ law A third law of thermodynamics A second law of thermodynamics A first law of thermodynamics In some systems which are used in pharmaceutical technology volume does not changes. What is kind of the correlation among internal energy and enthalpy in such systems? U = 2H 2U = 2H ?U > ?H ?U < ?H ?U = ?H What is the process according to this reaction of H2(g)+ Cl2(g) > 2HCl(g) + Q= -ΔH: Intencive Extensive Adiabatic Endothermic Exothermic Enthalpy is measured in: kkal/K kJ/molK kkal kJ kJ/mol What are the intensive properties of the thermodynamics system: Initial energy Concentration Internal energy Volume Mass What is the function that doesn’t depend on the passing way of a reaction but depends on the initial and the final state of a system? Volume B. C. * D. E. 139. A. B. * C. D. E. 140. A. B. C. * D. E. 141. A. B. C. D. * E. 142. A. B. C. * D. E. 143. A. B. C. D. * E. 144. A. * B. C. D. E. 145. A. B. C. * D. E. Pressure Enthalpy Work Heat Process, when there is V constant is ... Isothermal Isochoric Isobaric Isochoric– isothermal Isobaric– isothermal Open thermodynamic systems are exchanged with an environment: By nothing By components By a matter and energy By energy By a matter How can you classify thermodynamics systems according to their phases? Irreversible and reversible equilibrium and unequilibrium Isolated, opened, closed Homogeneous and heterogeneous Solid, liquid, gaseous Standard condition are when the values of pressure and temperature equal: 50 kPа, 298 K 50 kPа, 273 K 101,3 kPа, 298 K 101,3 kPа, 273 K 101,3 kPа, 0 K When the pressure and the volume are constant. What is name of this thermodynamic process? Isothermal Isochoric Isobaric Isobaric – isochoric Isochoric– isothermal Calcium has.... bond: Metallic Nonpolar covalent Polar covalent Hydrogen Ionic Hydrogen has ionic bond in compound: C2H2 CH4 CsH HCl H2 146. A. B. C. D. E. * 147. A. B. * C. D. E. 148. A. B. C. * D. E. 149. A. B. C. D. * E. 150. A. B. C. D. E. * 151. A. B. C. * D. E. 152. A. B. C. * D. E. 153. A. B. C. Oxygen has nonpolar covalent bond in compound: СО CaO K2O CO2 O2 The greatest electronegativity has element: Li Cl Br P Si All compounds have ionic bond: H2S, K2S SO2, H2SO3 NaCl, KCl Cl2, SO2 HCl, HBr All compounds have nonpolar covalent bond: NaCl, H2O, H2S H2SO4, K2SO4 NaCl, KCl N2, O2, Br2 HCl, HBr, H2O All compounds have polar covalent bond: NaCl, Cl2, H2 H2SO4, K2SO4 NaCl, KCl Cl2, H2, Br2 HCl, HBr, H2O What molecule has multiple bonds? I2 HCl N2 H2 polar molecule The most polar is ….bond: Hydrogen Metallic Ionic Nonpolar covalent Polar covalent Intermolecular hydrogen bond is between molecules of: F2 K2S N2 D. E. * 154. A. B. C. D. * E. 155. A. * B. C. D. E. 156. A. B. * C. D. E. 157. A. B. C. * D. E. 158. A. B. C. D. E. * 159. A. B. C. * D. E. 160. A. B. * C. D. E. 161. A. H2 HF Between water molecules is…. bond Metallic Nonpolar covalent Polar covalent Hydrogen Ionic All compounds have polar covalent bond except: O3 NH3 HF H2O H2SO4 What molecule has nonpolar covalent bond? NO H2 HF H2O H2SO4 Choose a compound which has nonpolar covalent bond is: Cu H2S F2 H2O K2O Choose a compound which has ionic bond is: Cu H2S F2 H2O K2O How many periods are in the periodical table of D. Mendeleev? 6 8 7 4 3 How many are groups in periodical table of D. Mendeleeva? 6 8 9 4 5 The greatest nonmetallic properties has: S B. C. D. * E. 162. A. B. C. D. * E. 163. A. B. C. D. E. * 164. A. B. * C. D. E. 165. A. B. C. D. * E. 166. A. * B. C. D. E. 167. A. * B. C. D. E. 168. A. B. C. D. E. * Na Cl .F Ag The greatest metallic properties has: Li Na Cl Fr F How many electrons are at f-lever? 8 10 16 6 14 How many electrons are at d-lever? 8 10 16 6 2 How many electrons are at p-lever? 7 32 16 6 2 How many electrons are at s-orbital? 2 32 16 8 3 The smallest unit of a chemical element that has the properties of that element is called: Atom Molecule Nucleon Electron Neutron What is spin? Type of hybridization Electronic orbitales Charge of nucleus of atom Electronic density Own motion of electron is about axis 169. A. B. C. D. * E. 170. A. B. C. * D. E. 171. A. B. C. * D. E. 172. A. * B. C. D. E. 173. A. B. C. D. * E. 174. A. B. * C. D. E. 175. A. B. C. D. * E. 176. A. B. * Two or more atoms having the same atomic number but differing in atomic weight and mass number is named: Protons Isochors Isotones Isotopes Spin Five electrons on a p electronic level have an atom: Argon Neon Fluorine Nitrogen Carbon The atomic mass is determined as: Sum mass of all electrons which are in atom Sum mass of neutrons which are in nucleus Sum mass of all protons and neutrons which are in nucleus Sum mass of all electrons which are in main electronic levels Sum mass of protons which are in nucleus What particle is influence for charge of atomic nucleus? Amount of protons Amount of electrons Common amount of nucleons Amount of neutrons Amount of positrons What particle is not in the atomic nucleus? Any one Proton Nucleon Electron Neutron Non-salts forming oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Amphoteric oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Complex substances are all except: HCl Cl2 C. D. E. 177. A. B. C. * D. E. 178. A. B. C. D. E. * 179. A. B. C. D. E. * 180. A. B. C. D. * E. 181. A. B. C. * D. E. 182. A. * B. C. D. E. 183. A. * B. C. D. E. 184. Fe(OH)3 MgO BaCO3 Acidic oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Basic oxides are: CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO CO, N2O, NO, SiO, H2O SO2; SO3; P2O5; Mn2O7; CrO3 ZnO; Al2O3; Cr2O3; SnO2 Na2O; MgO; CuO Salts are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3, CaCl2, MgCl2, Na3PO4,Ca3(PO4)2 Oxides are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Bases are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Acids are: HCl, HBr, H2S, HNO3, H3PO4 C, Cl2, KOH, CuO, H2SO4, NaH CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2 MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3 BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2 Complex salts are: [Ag(NH3)2]Br, Na[Ag(CN)2] NaHCO3, Na2HPO4 CaOCl2, KAl(SO4)2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Mixed salts are: A. B. C. * D. E. 185. A. B. C. D. E. * 186. A. * B. C. D. E. 187. A. B. * C. D. E. 188. A. B. C. D. * E. 189. A. B. C. * D. E. 190. A. B. * C. D. E. 191. A. * B. C. KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Basic salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Double salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Acidic salts are: KAl(SO4)2 NaHCO3, Na2HPO4 CaOCl2 Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Medium salts are: KAl(SO4)2 NaHCO3, Na2HPO4 Zn(OH)Cl Na2SO4, CaCl2 Zn(OH)Cl, Al(OH)2Br Mixed salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical. Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and ions of acid radical Basic salts are: In the time of dissociation gives two cations and one anion Under the dissociation give metal cations, hydroxyl anions and anions of acid Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid In the time of dissociation give only metal cations (or NH4+) and ions of acid Double salts are: Two cations and one anion are created during dissociation In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions D. E. 192. A. B. C. D. * E. 193. A. B. C. D. E. * 194. A. * B. C. D. E. 195. A. B. * C. D. E. 196. A. B. C. * D. E. 197. A. B. C. D. * E. 198. A. B. * In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and ions of acid radical Acidic salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+ ) and ions of acid radical Medium salts are: In the time of dissociation gives two cations and one anion In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical Formed by means of one cation and two anions In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid radical In the time of dissociation give only metal cations (or NH4+) and anions of acid radical Salts are: Complex substances, which consist from atoms of metal and acid residuals Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Acids are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting of hydrogen cations and anion Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which is oxygen Compound which molecules consist of one-type atoms Bases are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Oxides are: Complex substances, which consist from atoms of metal and acid residuals. This the most multiple class of inorganic compounds Complex substances, consisting from hydrogen atoms Complex substances, in which atoms of metals bonded with one or several hydroxyls groups Complex substances, consisting from two elements, one of which oxygen Compound which molecules consist of one-type atoms Monoatomic compound is: Water Helium C. D. E. 199. A. B. C. * D. E. 200. A. B. C. D. E. * 201. A. B. C. D. * E. 202. A. B. C. D. * E. 203. A. * B. C. D. E. 204. A. B. C. D. * E. 205. A. B. C. D. E. * 206. Ozone Ammonia Oxygen Such compound has three atoms in molecule: Aluminum hydride Hydrogen fluorine Hydrogen sulfur Ammonia Methanol Formula of molecule is: ОН3O 2O O-2 O2 Molar mass of sulfuric acid is: 49 g/mole 80 g/mole 106 g/mole 98 g/mole 65 g/mole Mass of three mole of water is: 6g 36 g 48 g 54 g 18 g Relative atomic mass of carbon is: 12 14 6 10 18 Molar mass of water is: 18 g 17 g/mole 24 g/mole 18 g/mole 16 g/mole Relative atomic mass of Oxygen is: 8 15 12 18 16 Molar volume at normal stat (a temperature 273 K and pressure of 101,3 kPa) has: A. B. * C. D. E. 207. A. B. C. * D. E. 208. A. B. C. * D. E. 209. A. B. C. D. E. * 210. A. * B. C. D. E. 211. A. B. C. D. E. * 212. A. B. C. * D. E. 22,4 m3 22,4 l/mol 11,2 l/mole lest then 22,4 l/mole more than 22,4 l/mole During the physical phenomena: There is a change of quantitative composition of compound There is a change of amount of electrons in an atom There is a change of the aggregate state of compound There is a change only of chemical elements There is a change of qualitative composition of molecules 112 g of nitrogen have volume: 56,9 l 11,2 l 89,6 l 112 l 22,4 l Complex compound: О3 C О2 H2 СО2 Choose correct definition “simple compound is…..” molecules or crystals are contain atoms of one element molecules or crystals are contain atoms of 3th different elements molecules or crystals are contain atoms of one group elements molecules or crystals are contain atoms of 2th elements molecules or crystals are contain atoms of different elements To choose oxygen-containing acids: H2S HBr HCl HI H2SO4 To choose the simple compound: HNО3 CO О2 H2O СО2