Textbook Question
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O2(g) + 2 H2O(l) + 4 Ag(s) → 4 OH–(aq) + 4 Ag+(aq) b. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
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Ch.19 - Electrochemistry
Chapter 19, Problem 64
Which of the following metals is the best reducing agent? a. Mn b. Al c. Ni d. Cr
Verified step by step guidance1
insert step 1> Identify the concept of a reducing agent. A reducing agent is a substance that loses electrons and is oxidized in a chemical reaction.
insert step 2> Consider the standard reduction potentials for each metal. The more negative the reduction potential, the better the metal is at losing electrons, making it a better reducing agent.
insert step 3> Look up the standard reduction potentials for each metal: Mn, Al, Ni, and Cr.
insert step 4> Compare the reduction potentials. The metal with the most negative reduction potential is the best reducing agent.
insert step 5> Determine which metal has the most negative reduction potential and conclude that it is the best reducing agent among the options provided.
Related Practice
Textbook Question
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO2(s) + 4 H+(aq) + Sn(s) → Pb2+(aq) + 2 H2O(l) + Sn2+(aq)
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Textbook Question
Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+
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Textbook Question
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. b. Br2(l) + 2 Cl–(aq) → 2 Br–(aq) + Cl2(g) c. MnO2(s) + 4 H+(aq) + Cu(s) → Mn2+(aq) + 2 H2O(l) + Cu2+(aq)
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Textbook Question
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn2+(aq) b. O2(g) + 2 H2O(l) + 2 Cu(s) → 4 OH–(aq) + 2 Cu2+(aq) c. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
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Textbook Question
Calculate the equilibrium constant for each of the reactions in Problem 65.
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