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Super-Quiz QF-B Gertz-Ressler High School Chemistry 2 DO NOT write on the booklet Standard 4: Gases 1. (4.a) In the following diagram, what is the relationship observed between the variables? 5. (4.a) According to the Kinetic theory, pressure over a wall is caused by: a) Particles colliding against the wall b) Gravity c) Water vapor d) Activation energy 6. (4.f) What is Zero absolute? a) 32oF b) 0oC c) -273 K a) Temperature increases, volume decreases b) Volume decreases, pressure increases c) Volume increases, temperature increases d) None 2. (4.a) According to the Kinetic theory, if the temperature in a gas system increases, the gas particles will move faster. Choose the correct statement below: a) If the temperature increases and the volume stays the same, the pressure increases. b) If the temperature increases and the volume stays the same, the pressure decreases. c) If the temperature increases and the pressure increases, the number of moles of particles also increases. d) If the temperature increases and the volume increases, the pressure increases. 3. (4.e) Convert 70oC to Kelvin? a) -70 K b) 343 K c) 203 K d) 373 K 4. (4.c) What is the volume of 2 moles of gas at STP? a) 44.8 L b) 11.2 L c) 22.4 L d) 30 L d) 0 K 7. (4.d) What is “STP conditions”? a) P = 1 atm, T = 0 oC b) P = 1 atm, T = 0 oF c) P = 0 atm, T = 0 oC d) P = 1 atm, T = 25 oC 8. (4.i) Dalton’s Law says that the total pressure of a mixture of gases is: a) 1 atm b) The sum of all the partial pressures of the gases c) Variable d) None Standard 5: Acids, Bases and Salts 9. (5.a) The correct formula for hydrofluoric acid is: a) HFO4 b) HF c) H4F d) HFO3 10. (5.a) The taste of acids is a) sweet b) sour c) bitter d) salty 11. (5.d) An acidic solution has a pH that is a) more than 7 b) = 7 c) less than 7 d) any value 12. (5.d) A neutral solution a) completely dissociates in water b) partially dissociates in water c) has a pH = 7 d) changes color 13. (5.c) A strong acid a) partially dissociates in water b) completely dissociates in water c) changes color d) has a pH = 7 19. (6.a) What is a chemical solution? a) any mixture b) heterogeneous mixture c) homogeneous mixture d) non-polar substance 14. (5.a) A neutralization reaction between an acid and a base always produces a) water and salt b) water and basic anhydride c) salt and basic anhydride d) salt and acidic anhydride 20. (6.d) How many moles of CaCO3 are needed to prepare 5.0 liters of a 2.0 M solution of CaCO3? a) 5 moles b) 10 moles c) 20 moles d) none 15. (5.b) Arrhenius defines an acid as a substance that a) donates H+ b) donates OHc) accepts H+ d) accepts OH16. (5.c) Complete the dissociation of HBr HBr + H2O ________ + _________ a) H2Br + HOc) HBr2- + O+ b) Br- + H3O+ d) BrO- + HO+ 17. (5.a) Rolaids®, active ingredient: Mg(OH)2, is the name of _________ used to fight high _________ . a) gas, indigestion b) salt tablets, fever c) acid tablets, alkalinity d) base tablets, acidity Standard 6: Chemical Solutions 18. (6.a) What is a solute? a) any substance b) medium that dissolves a substance c) substance being dissolved d) mixture of substances 21. (6.a) A saturated solution has a __________ amount of solute. a) less than maximum b) maximum possible c) more than maximum d) none 22. (6.a) What is the meaning of aqueous solution? a) The solution is ionic b) The solute is water c) The solution is an electrolyte d) The solvent is water 23. (6.b) When 1 mol of K2SO4 dissociates in water, it produces ______ of K+ ions. (Balance the equation first) a) 1 mol __ K2SO4 __ K+ + __ SO4b) 2 moles c) 3 moles d) 4 moles 24. (6.b) Chemists often say “like dissolves like.” What does this statement mean? a) A substance will dissolve always b) Polar/Ionic solvent dissolves polar/ionic solute c) Something dissolves like salt d) It is likely that the solute will dissolve 25. (6.c) Generally, the rate of dissolution of a solid in a liquid increases when the temperature _________. a) Increases b) Decreases c) Is constant d) is Standard 26. (6.d) What is the mass % of solute in a solution that contains 30g of solute and 30g of water? a) 100% b) 50% c) 30% d) none Standard 7: Chemical Thermodynamics 27. (7.c) When water changes phase from liquid to gas, the process is a) Exothermic b) Endothermic c) Neutral d) Kinetic 28. (7.c) The temperature of iced water melting is _____ oC. The temperature of boiling water is _____ oC. a) 100, 200 b) 0, 100 c) 100, 0 d) None 29. (7.b) If in a chemical reaction, the products have more potential energy than the reactants, the reaction is… a) Exothermic b) Endothermic c) Neutral d) Kinetic 30. (7.d) A substance was tested for its behavior when heated. It was first a solid; then by adding energy it warmed-up and melted, then more heat was added so it warmed-up more and boiled. The following graph of temperature was obtained: 32. (7.a) Temperature is the measure of … a) The chemical bonds in a substance b) The pressure of a gas c) The actual size of the molecules d) The kinetic energy of the particles in a substance 33. (7.b) A sample ofwater changes temperature from 56 oC to 20 oC. This process is a) Exothermic b) Endothermic c) Neutral d) Kinetic 34. (7.d) Problem. Use the same set of formulas and constants. You want to evaporate 400.0 g of water. Calculate the amount of heat needed. (Hv of water = 2,256 J/g) a) 1,128,000 J b) 400 J c) 902,400 J d) 2,256 J 35. (7.d) Problem. Use the formulas and constants below. You want to heat 400.0 g of water from 20oC to 65 oC. Calculate the amount of heat needed. (Cp of water = 4.18 J/goC) a) 400.0 J b) 75,240 J c) 19,176 J d) 52,250 J 135 Formulas 92 o C -12 -40 Energy, Joules -40 From the graph, the liquid was warmed-up from ______ to ______ oC. a) -40, -12 b) -12, 92 c) 92, 135 d) -40, 92 31. (7.a) Heat flows from a _______ to a _______ body. a) Soft, Hard b) Cold, Hot c) Big, Small d) Hot, Cold Sensible heat: Q = m Cp ΔT Change of temperature: Latent heat (evaporation): Latent heat (evaporation): ΔT = T2 – T1 Q= m Hv Q= m Hf Constants for water Heat capacity: Cp(water) = 4.18 J/g oC Latent heat (vaporization): Hv(water) = 2,256 J/g Latent heat (fusion): Hf(water) = 333 J/g Std 8: Rate of Reaction 36. (Std 8) The energy required to start a reaction is called… a) Energy of reaction b) Released energy c) Energy of activation d) Energy of catalyst 37. (Std 8) A change in concentration of reactants or products over time is the: a) Activated complex b) Transition state c) Reaction rate d) Intermediate product 38. (Std 8) Catalysts... a) Slow the rate of a reaction b) Increase the energy of the reactants c) Lower the activation energy d) Are used up in reactions 39. (Std 8) For a reaction to take place, the molecules need both to: a) be acid, and base b) be ionic, and covalent c) collide with enough energy, and with correct orientation d) None of the above 40. (Std 8) For a particular reaction, rate = k[A]2[B][C]3 If the concentration of reactant B is doubled, the rate is increased by a factor of: a) 2 b) 4 c) 1/2 d) 1/4 41. (Std 8) Consider the following reaction in the gas phase: N2O4 (g) 2NO2 (g) If you increase the pressure over this system, the rate of reaction will a) Decrease b) Increase c) Stop d) Doesn’t affect Std 9: Chemical Equilibrium 42. (Std 9) Choose the expression for k, the equilibrium constant, for the reaction: 2NO2 (g) N2O4 (g) a) [ N2O4 ] K= ----------------[ NO2 ] 2 [ NO2 ] 2 b) K = -------------------[ N2O4 ] c) [ N2O4 ] 2 K= ----------------[ NO2 ] d) K = [ NO2 ] 2 [ N2O4 ] 43. (Std 9) LeChatelier’s principle establishes that: a) The reactants are the same as the products b) Equilibrium is a stress c) A system will act in order to re-establish equilibrium d) The reactants are at the left side Std 10: Organic Chemistry 44. A molecule of hexene has a) only single bonds between carbons b) a carbon-carbon double bond c) a carbon-carbon triple bond d) a hexagonally shaped ring structure 45. What functional group contains a hydrocarbon which ends in OH? a) alcohol b) ketone c) ether d) amine 46. Which compounds have carbon-carbon double bonds? a) alkanes b) alkenes c) alcohols d) ionic compounds 47. The simplest organic compound is a) aspirin b) table sugar c) salt d) methane 48. Polymers are large organic molecules that are made of a) cations b) anions c) carbon and oxygen only d) repeating units 49. Protein molecules are complex polymer molecules made up of repetitive monomers called a) nitrogenous bases b) amino acids c) simple sugars d) vitamins 50. What is the name of a hydrocarbon containing a 6-carbon chain? a) pentane b) propane c) hexane d) heptane 51. Alkanes are hydrocarbons that contain a) single covalent bonds only b) single or double covalent bonds. c) carbon and oxygen only d) carbon, hydrogen, and oxygen. 52. Alcohols are organic compounds that contain a) carbon and oxygen only b) carbon and hydrogen only c) carbon, oxygen, and hydrogen d) carbon, nitrogen, and hydrogen 53. Carbon can form a large variety of compounds from simple to highly complex due to its ability to a) form ions with four different charges b) form four covalent bonds c) share electrons with itself d) form ionic bonds with many elements 54. The name of hydrocarbon compounds, such as methane, contains two parts: a prefix (meth) and a suffix (ane). The prefix tells a) the number of hydrogen atoms present b) the number of carbon atoms present c) whether single, double or triple C-C bonds are present d) whether the molecule is a straight-chain or a ring Std 11: Nuclear Chemistry 55. The decay of C-14 is used as a tool for… a) X-Rays b) Making fuel c) Dating fossil samples d) Making organic compounds 56. Complete the following nuclear equation: 239 __ Np ___ 93 a) 0 239 Th 90 b) 239 92 U e + __ -1 c) 239 Pu 94 d) 238 Pu 94 57. The most abundant isotope of lead contains 82 protons and 124 neutrons packed closely together in the nucleus. Why do the protons stay together in the nucleus rather than fly appart? a) Electrons in neighboring atoms neutralize repulsive forces between protons. b) Nuclear forces overcome repulsive forces between protons in the nucleus. c) Electrostatic forces between neutrons and protons hold the nucleus together. d) Neutrons effectively block the protons and keep them far apart to prevent repulsion. 58. A 2 cm thick piece of cardboard placed over a radiation source would be most effective in protecting against which type of radiation? a) Alpha b) Beta c) Gamma d) X-ray 59. Which of the following lists ranks nuclear radiation from most massive to least massive? a) alpha, beta, and gamma b) beta, gamma, and alpha c) gamma, alpha, and beta d) gamma, beta, and alpha 60. What is the half-life of an isotope if 40 g of a 320 g sample of the isotope remains after 18.0 years? a) 1.0 years b) 3.0 years c) 6.0 years d) 9.0 years 61. A big nucleus splitting into two smaller ones, accompanied by a great emission of energy, is a) nuclear fusion b) nuclear fission c) nuclear power d) nuclear radiation 62. Complete the following nuclear equation: 238 __ U 4 2 He U ____ + 92 a) 239 __ b) 1 0 n c) 92 1 1 H d) 0 -1 e 63. The time it takes for ½ of a sample of radioactive material to decay is… a) Average life b) Expected life c) Half-life d) Decay time ***END OF TEST, STOP AND REVIEW*** QFGR2B.doc J. Bermudez