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Question 1

Question 1. Identify the species that is oxidized and the species that is reduced in the reaction: 2 I – + Cl 2  2 Cl – + I 2 A) I – is oxidized and Cl 2 is reduced . B ) Cl 2 is oxidized and I – is reduced . C) I 2 is oxidized and Cl – is reduced .

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Question 1

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  1. Question 1 Identify the species that is oxidized and the species that is reduced in the reaction: 2 I– + Cl22 Cl– + I2 A) I– is oxidized and Cl2 is reduced. B) Cl2 is oxidized and I– is reduced. C) I2 is oxidized and Cl–is reduced. D) Cl2 is oxidized and Cl–is reduced. E) I2 is oxidized and I–is reduced.

  2. Question 1 Identify the species that is oxidized and the species that is reduced in the reaction: 2 I– + Cl22 Cl– + I2 A) I– is oxidized and Cl2 is reduced. B) Cl2 is oxidized and I– is reduced. C) I2 is oxidized and Cl–is reduced. D) Cl2 is oxidized and Cl–is reduced. E) I2 is oxidized and I–is reduced.

  3. Question 2 What is the expression for the equilibrium constant for the reaction 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)? A)K= [CO2][H2O] B) K = [CO2]4[H2O]6 [C2H6][O2] [C2H6]2[O2]7 C) K= [C2H6][O2] D) K = [C2H6]2[O2]7 [CO2][H2O] [CO2]4[H2O]6

  4. Question 2 What is the expression for the equilibrium constant for the reaction 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)? A)K= [CO2][H2O] B) K = [CO2]4[H2O]6 [C2H6][O2] [C2H6]2[O2]7 C) K= [C2H6][O2] D) K = [C2H6]2[O2]7 [CO2][H2O] [CO2]4[H2O]6

  5. Question 3 The definition of a Brønsted-Lowry acid is: A) a compound that contains hydroxide and dissolves in water to form –OH. B) a compound that is a proton donor. C) a compound that is a proton acceptor. D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

  6. Question 3 The definition of a Brønsted-Lowry acid is: A) a compound that contains hydroxide and dissolves in water to form –OH. B) a compound that is a proton donor. C) a compound that is a proton acceptor. D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

  7. Question 4 An alpha particle is a high-energy particle that contains: A) one proton and one neutron. B) two protons and two neutrons. C) one electron. D) one proton.

  8. Question 4 An alpha particle is a high-energy particle that contains: A) one proton and one neutron. B) two protons and two neutrons. C) one electron. D) one proton.

  9. Question 5 In the balanced redox reaction: 2 Cu(s) + S(s)  Cu2S(s) how many electrons are gained or lost by each sulfur atom? A) each sulfur atom gains two (2) electrons B) each sulfur atom gains one (1) electron C) each sulfur atom loses one (1) electron D) each sulfur atom loses two (2) electrons

  10. Question 5 In the balanced redox reaction: 2 Cu(s) + S(s)  Cu2S(s) how many electrons are gained or lost by each sulfur atom? A) each sulfur atom gains two (2) electrons B) each sulfur atom gains one (1) electron C) each sulfur atom loses one (1) electron D) each sulfur atom loses two (2) electrons

  11. Question 6 An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium A) the reactants are favored. B) the products are favored. C) approximately equal concentrations of reactants and products are present.

  12. Question 6 An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium A) the reactants are favored. B) the products are favored. C) approximately equal concentrations of reactants and products are present.

  13. Question 7 Which species can be a Brønsted–Lowry acid? A) CO32– B) HBr C) Br2 D) LiOH

  14. Question 7 Which species can be a Brønsted–Lowry acid? A) CO32– B) HBr C) Br2 D) LiOH

  15. Question 8 Which species is the conjugate acid of HCO3–? A) CO32– B) H2CO3 C) CO2 D) H2O

  16. Question 8 Which species is the conjugate acid of HCO3–? A) CO32– B) H2CO3 C) CO2 D) H2O

  17. Question 9 Which is the symbol for the beta particle? A) 1e 0 B) 1e -1 C) 0e -1 D) 0e 1

  18. Question 9 Which is the symbol for the beta particle? A) 1e 0 B) 1e -1 C) 0e -1 D) 0e 1

  19. Question 10 In the balanced redox reaction: 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g), which species is reduced? A) C2H6(g) B) O2(g) C) CO2(g) D) H2O(g)

  20. Question 10 In the balanced redox reaction: 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g), which species is reduced? A) C2H6(g) B) O2(g) C) CO2(g) D) H2O(g)

  21. Question 11 In the galvanic cell created using zinc and copper placed in zinc sulfate and copper (II) sulfate solutions respectively, which species forms the anode of the cell? A) Zinc B) Zinc sulfate C) Copper D) Copper sulfate Reduction ReactionE0 (v) Zn2+ (aq) + 2e- Zn (s) -0.76 Cu2+ (aq) + 2e-  Cu (s) +0.34

  22. Question 11 In the galvanic cell created using zinc and copper placed in zinc sulfate and copper (II) sulfate solutions respectively, which species forms the anode of the cell? A) Zinc B) Zinc sulfate C) Copper D) Copper sulfate Reduction ReactionE0 (v) Zn2+ (aq) + 2e- Zn (s) -0.76 Cu2+ (aq) + 2e-  Cu (s) +0.34

  23. Question 12 What is the correct cell notation for the zinc/copper cell described in the previous question? A) Cu|Zn||Cu2+|Zn2+ B) Cu|Cu2+||Zn2+|Zn C) Zn|Zn2+||Cu2+|Cu D) Zn2+|Zn||Cu|Cu2+ Reduction ReactionE0 (v) Zn2+ (aq) + 2e- Zn (s) -0.76 Cu2+ (aq) + 2e-  Cu (s) +0.34

  24. Question 12 What is the correct cell notation for the zinc/copper cell described in the previous question? A) Cu|Zn||Cu2+|Zn2+ B) Cu|Cu2+||Zn2+|Zn C) Zn|Zn2+||Cu2+|Cu D) Zn2+|Zn||Cu|Cu2+ Reduction ReactionE0 (v) Zn2+ (aq) + 2e- Zn (s) -0.76 Cu2+ (aq) + 2e-  Cu (s) +0.34

  25. Question 13 For an endothermic reaction, increasing the temperature A) does not shift the equilibrium since K is a constant. B) increases the rate of the reverse reaction to form more reactants. C) increases the rate of the forward reaction to form more products. D) increases the rate of the reverse reaction to form more products.

  26. Question 13 For an endothermic reaction, increasing the temperature A) does not shift the equilibrium since K is a constant. B) increases the rate of the reverse reaction to form more reactants. C) increases the rate of the forward reaction to form more products. D) increases the rate of the reverse reaction to form more products.

  27. Question 14 Which acid is the strongest? A) Hydrogen sulfate ion HSO4– (Ka = 1.2 x10–2) B) Hydrocyanic acid HCN (Ka = 4.9 x10–10) C) Hydrofluoric acid HF (Ka = 7.2 x10–4) D) Ammonium ion NH4+ (Ka = 5.6 x10–10)

  28. Question 14 Which acid is the strongest? A) Hydrogen sulfate ion HSO4– (Ka = 1.2 x10–2) B) Hydrocyanic acid HCN (Ka = 4.9 x10–10) C) Hydrofluoric acid HF (Ka = 7.2 x10–4) D) Ammonium ion NH4+ (Ka = 5.6 x10–10)

  29. Question 15 If the half-life of phosphorus-32 is 14 days, how much of a 300. mg sample of phosphorus-32 remains after 56 days? A) 150. mg B) 37.5 mg C) 18.8 mg D) 9.38 mg

  30. Question 15 If the half-life of phosphorus-32 is 14 days, how much of a 300. mg sample of phosphorus-32 remains after 56 days? A) 150. mg B) 37.5 mg C) 18.8 mg D) 9.38 mg

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