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18 Nov 2019
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Standard Reduction Potential Half Reaction EO, Volts Ca2+ (aq) 2 e Ca (s) 2.87 Mn2+ (aq) 2 e Mn (s) 1.18 Co2 (aq) 2 e Co (s) 0.28 2 H+ (aq) 2 e H2 (g) 0.00 +0.80 Ag+ (aq) e Ag (s) Cl2 (g) 2 e 2Cl- (aq) +1.36 1. c u ,,etion potentials above, a 1,
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Electrochemical Cells DATE SECTION Standard Reduction Potential Half Reaction E Volts Ca (aq) 2 e- Can (s) 2.87 Mnz (aq) 2e. Mn (s) 1.18 Co (aq) 2 e Co (s) 2 H+ (aq) 2 e H2 (g) -0.00 Ag+ (aq) e. Ag (s) +0.80 Clz (g) 2 e 2Cl (aq) 1.36 Given the partial list of standard reduction potentials above, answer Questions 1-5. 1. Will calcium (Ca) spontaneously reduce silver ion (Ag+) to silver (Ag Briefly explain your answer. If yes, what is E PRELA
Ca^2+ (aq) + 2 e^- rightarrow Ca (s) -2.87 Mn^2+ (aq) + 2 e^- rightarrow Mn (s) -1.18 Co^2+ (aq) + 2 e^- rightarrow Co (s) -0.28 2 H^+ (aq) + 2 e^- rightarrow H_2 (g) -0.00 Ag^+ (aq) + e^- rightarrow Ag (s) +0.80 Cl_2 (g) + 2 e^- rightarrow 2 Cl^- (aq) + 1.36 Will silver metal react spontaneously with HCl (aq) to produce H_2 (g) ? Briefly explain. What is the cell potential for the Mn/Mn^2+ | | Co^2+/Co cell, based on the standard potentials given above? Will the reaction between Ca^2+ and Cl^- ions to form Ca metal and Cl_2 (g) be spontaneous ? Briefly explain. A student constructed a Mg/Mg^2+ | | Ag^+/Ag cell and measured a cell potential of 3.17 volts. Calculate the reduction potential of the Mg/Mg^2+ half-reaction.
omework m 8 Which of these redox reactions do you expect to occur spontaneously in the forward direction? Standard Electrode Potentials at 25 ° C Reduction Half-Reaction Ni2+ (aq) + 2 e-â Ni(s) Zn2+ (aq) + 2e-âZn(s) Cd2+ (aq) + 2 e-â Cd(s) Co2+ (aq) + 2 e-â Co(8) PbH (aq) + 2 e-âPb(s) Fe2+ (aq) + 2 e-â Fe(s) AP+ (aq) + 3 e-âAl(s) Ag+ (aq) + e-âAg(s) Cr3+ (aq) + 3 e-â Cr(s) Mn2+ (aq) +2 e-âMn(8) Eo (V) -023 -0.76 -0.40 -0.28 -0.13 -045 -1.66 0.80 -0.73 -1.18 Check all that apply â¡ Fe2+ (aq) + Zn(s)âFe(s) +m2+ (aq) â¡ Pb(s) + Mn2+ (aq) â Pb2+ (aq) + Mn(a) â¡ Ni(s) + Zn2+ (aq) â Ni2+ (aq) + Zn(s) â¡ Cr(s) + 3 Ag+ (aq) â Cr3+ (aq) + 3 Ag(s) Back-
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