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Answers to examination questions
... The oxygen molecule (OO) contains one double bond; the carbon dioxide molecule (OCO) contains two double bond and the tetrafluoroethene molecule contains one double bond. ...
... The oxygen molecule (OO) contains one double bond; the carbon dioxide molecule (OCO) contains two double bond and the tetrafluoroethene molecule contains one double bond. ...
Chemistry Entrance Material for Grade 11 to 12
... [-A-] The remaining liquid continues to become cooler because the molecules continue to evaporate all the time. [-B-] The liquid continues to cool down. [-C-] The liquid may cool down initially, but then it will stay at the same temperature because the system has reached equilibrium. [-D-] The remai ...
... [-A-] The remaining liquid continues to become cooler because the molecules continue to evaporate all the time. [-B-] The liquid continues to cool down. [-C-] The liquid may cool down initially, but then it will stay at the same temperature because the system has reached equilibrium. [-D-] The remai ...
atom - Zanichelli online per la scuola
... Dalton’s law of multiple proportions The law of multiple proportions states that when two elements combine to give more than one compound, the masses of one element that combine with the fixed mass of the other are in a ratio of small whole numbers. ...
... Dalton’s law of multiple proportions The law of multiple proportions states that when two elements combine to give more than one compound, the masses of one element that combine with the fixed mass of the other are in a ratio of small whole numbers. ...
State Standard - SchoolNotes.com
... units that reflect the precision and accuracy of each particular instrument. C-1.4 Design a scientific investigation with appropriate methods of control to test a hypothesis (including independent and dependent variables), and evaluate the designs of sample investigations. C-1.5 Organize and interpr ...
... units that reflect the precision and accuracy of each particular instrument. C-1.4 Design a scientific investigation with appropriate methods of control to test a hypothesis (including independent and dependent variables), and evaluate the designs of sample investigations. C-1.5 Organize and interpr ...
Chemistry 11 Review
... 8. Which of the following reactions is most likely to have the greatest rate at room temperature? a) Ag+(aq) + I- (aq) AgI(s) b) H2 (g) + Cl2 (g) 2HCl (g) c) C3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O (g) ...
... 8. Which of the following reactions is most likely to have the greatest rate at room temperature? a) Ag+(aq) + I- (aq) AgI(s) b) H2 (g) + Cl2 (g) 2HCl (g) c) C3H8 (g) + 5O2 (g) 3CO2 (g) + 4H2O (g) ...
Chemistry Final Exam Review
... 2. Complete the following reactions by giving the correct formulas for the products (there is no need to balance): a. P2O5 ...
... 2. Complete the following reactions by giving the correct formulas for the products (there is no need to balance): a. P2O5 ...
Stoichiometry – Chapter 9
... hydrochloric acid with pyrolusite [manganese dioxide or manganese(IV) oxide, MnO2], a common manganese ore. Small amounts of chlorine may be prepared in the laboratory by the same reaction. 4HCl(aq) + MnO 2 (s) → 2H 2 O(l) + MnCl 2 (aq) + Cl 2 (g) 3A. How many grams of HCl react with 5.00 g of MnO2, ...
... hydrochloric acid with pyrolusite [manganese dioxide or manganese(IV) oxide, MnO2], a common manganese ore. Small amounts of chlorine may be prepared in the laboratory by the same reaction. 4HCl(aq) + MnO 2 (s) → 2H 2 O(l) + MnCl 2 (aq) + Cl 2 (g) 3A. How many grams of HCl react with 5.00 g of MnO2, ...
Section 1 Describing Chemical Reactions Chapter 8
... CH4(g) + Al(OH)3(s) (not balanced) • Balance Al atoms Al4C3(s) + H2O(l) CH4(g) + 4Al(OH)3(s) (partially balanced) ...
... CH4(g) + Al(OH)3(s) (not balanced) • Balance Al atoms Al4C3(s) + H2O(l) CH4(g) + 4Al(OH)3(s) (partially balanced) ...
What is Thermodynamics?
... It may appear to be stable but diamonds forms at high P, T and, therefore, is only METASTABLE (appears stable) when sitting on the desk at STP. Predicting whether a phase spontaneously reacts is governed by the ENERGY of the SYSTEM (study of thermodynamics), But the actual RATE of REACTION is the st ...
... It may appear to be stable but diamonds forms at high P, T and, therefore, is only METASTABLE (appears stable) when sitting on the desk at STP. Predicting whether a phase spontaneously reacts is governed by the ENERGY of the SYSTEM (study of thermodynamics), But the actual RATE of REACTION is the st ...
Unit 3 Exam Level Questions
... A Increases the rate of the forward reaction only B Increases the rate of the reverse reaction only C Increases the rate of both the forward and reverse reactions D Changes the position of the equilibrium of the reaction 2. In which of the following systems will the equilibrium be unaffected by a ch ...
... A Increases the rate of the forward reaction only B Increases the rate of the reverse reaction only C Increases the rate of both the forward and reverse reactions D Changes the position of the equilibrium of the reaction 2. In which of the following systems will the equilibrium be unaffected by a ch ...
CIS Exam Questions
... A Increases the rate of the forward reaction only B Increases the rate of the reverse reaction only C Increases the rate of both the forward and reverse reactions D Changes the position of the equilibrium of the reaction 2. In which of the following systems will the equilibrium be unaffected by a ch ...
... A Increases the rate of the forward reaction only B Increases the rate of the reverse reaction only C Increases the rate of both the forward and reverse reactions D Changes the position of the equilibrium of the reaction 2. In which of the following systems will the equilibrium be unaffected by a ch ...
aq - Haverford Alchemy
... To determine if an oxidation-reduction reaction has occurred, we assign an oxidation number to each element in a neutral compound or charged entity. ...
... To determine if an oxidation-reduction reaction has occurred, we assign an oxidation number to each element in a neutral compound or charged entity. ...
Unit 1 Student Booklet
... more than one atom of each element in a binary compound. Binary ionic compounds usually contain one kind of metal ion combined with one kind of non-metal ion. Metal ions have positive charges and non-metal ions have negative charges. When naming an ionic compound from its formula, follow the rules b ...
... more than one atom of each element in a binary compound. Binary ionic compounds usually contain one kind of metal ion combined with one kind of non-metal ion. Metal ions have positive charges and non-metal ions have negative charges. When naming an ionic compound from its formula, follow the rules b ...
Unit - 7.pmd
... the absence of d orbitals in its valence shell. Besides restricting its covalency to four, nitrogen cannot form dπ –pπ bond as the heavier elements can e.g., R3P = O or R3P = CH2 (R = alkyl group). Phosphorus and arsenic can form dπ –dπ bond also with transition metals when their compounds like P(C2 ...
... the absence of d orbitals in its valence shell. Besides restricting its covalency to four, nitrogen cannot form dπ –pπ bond as the heavier elements can e.g., R3P = O or R3P = CH2 (R = alkyl group). Phosphorus and arsenic can form dπ –dπ bond also with transition metals when their compounds like P(C2 ...
View PDF
... ____ 24. In the equation 2Al(s) + 3Fe(NO 3 ) 2 (aq) → 3Fe(s) + 2Al(NO 3 ) 3 (aq), iron has been replaced by a. nitrate. c. aluminum. b. water. d. nitrogen. ____ 25. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the sol ...
... ____ 24. In the equation 2Al(s) + 3Fe(NO 3 ) 2 (aq) → 3Fe(s) + 2Al(NO 3 ) 3 (aq), iron has been replaced by a. nitrate. c. aluminum. b. water. d. nitrogen. ____ 25. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal originally in the sol ...
apchem - practice midterm_shs
... answers for Section I on the separate answer sheet. Use the test booklet for your scratch work or notes, but remember that no credit will be given for work, notes, or answers written only in the test booklet. Once you have selected an answer, blacken thoroughly the corresponding circle on the answer ...
... answers for Section I on the separate answer sheet. Use the test booklet for your scratch work or notes, but remember that no credit will be given for work, notes, or answers written only in the test booklet. Once you have selected an answer, blacken thoroughly the corresponding circle on the answer ...
XIX. Chemistry, High School
... Reference Materials and Tools Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question in this chapter. Each student also had sole access to a calc ...
... Reference Materials and Tools Each student taking the high school Chemistry test was provided with a Chemistry Formula and Constants Sheet/Periodic Table of the Elements. Copies of both sides of this formula sheet follow the final question in this chapter. Each student also had sole access to a calc ...
Document
... 110. Carbon dioxide gives milky color with limewater due to the formation of _____. A) CaO B) CaCO3 C) Ca(HCO3)2 D) Ca(OH)2 ...
... 110. Carbon dioxide gives milky color with limewater due to the formation of _____. A) CaO B) CaCO3 C) Ca(HCO3)2 D) Ca(OH)2 ...
Full Text PDF
... delocalization from atom is larger when spin-orbit coupling occurs. Measurements in progress suggest that the same conclusion is also tue for the complexes formed by the same metal ions with H 4 EDTA (ethylenediaminetetraacetic acid). ...
... delocalization from atom is larger when spin-orbit coupling occurs. Measurements in progress suggest that the same conclusion is also tue for the complexes formed by the same metal ions with H 4 EDTA (ethylenediaminetetraacetic acid). ...
Chem 11 Notes Booklet (pdf version)
... CaCO3 + energy CaO + CO2 The heat is much like a reactant – without it, the reaction cannot take place. ...
... CaCO3 + energy CaO + CO2 The heat is much like a reactant – without it, the reaction cannot take place. ...
Chem 171 Review - Exam 1
... Hematite, Fe2O3, is an important ore of iron. Iron metal is obtained by reacting hematite with carbon monoxide (CO) in a blast furnace. The balanced chemical equation for this reaction is: Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g) Calculate the mass (in g) of iron that can be produced from the com ...
... Hematite, Fe2O3, is an important ore of iron. Iron metal is obtained by reacting hematite with carbon monoxide (CO) in a blast furnace. The balanced chemical equation for this reaction is: Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g) Calculate the mass (in g) of iron that can be produced from the com ...
2012 C13 Exam answers
... 32 Which statement about catalysts is incorrect? 28 A cylinder of unknown volume contains helium gas, He(g), at 3.50 atm and 315 K. The helium gas is then transferred to a 7.0 L gas cylinder containing Ne(g), at 2.50 atm and 315 K. If the final total pressure at 315 K is 5.75 atm, then what is the v ...
... 32 Which statement about catalysts is incorrect? 28 A cylinder of unknown volume contains helium gas, He(g), at 3.50 atm and 315 K. The helium gas is then transferred to a 7.0 L gas cylinder containing Ne(g), at 2.50 atm and 315 K. If the final total pressure at 315 K is 5.75 atm, then what is the v ...
Environmental Chemistry
... (a) for aerobic water having a pE = +11, and (b) for anaerobic water with pE = -3 pE = 14.15 – (5/4)pH – (1/8)log([NH4+] / [NO3-]) 11 = 14.15 – (5/4) x 6 – (1/8)log([NH4+] / [NO3-]) log([NH4+] / [NO3-]) = -8(4.35) = -34.8 [NH4+] / [NO3-] = 1.6 x 10-35 pE = 14.15 – (5/4)pH – (1/8)log([NH4+] / [NO3-]) ...
... (a) for aerobic water having a pE = +11, and (b) for anaerobic water with pE = -3 pE = 14.15 – (5/4)pH – (1/8)log([NH4+] / [NO3-]) 11 = 14.15 – (5/4) x 6 – (1/8)log([NH4+] / [NO3-]) log([NH4+] / [NO3-]) = -8(4.35) = -34.8 [NH4+] / [NO3-] = 1.6 x 10-35 pE = 14.15 – (5/4)pH – (1/8)log([NH4+] / [NO3-]) ...
Redox
![](https://commons.wikimedia.org/wiki/Special:FilePath/NaF.gif?width=300)
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.