Textbook Question
The following cell reactions occur spontaneously: (a) Arrange the following reduction half-reactions in order of decreasing tendency to occur:
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Ch.19 - Electrochemistry
Chapter 19, Problem 80b
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni2+(aq) by Sn2+(aq)
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Identify the half-reactions involved in the process. For the reduction of Ni^{2+}(aq), the half-reaction is: Ni^{2+}(aq) + 2e^- \rightarrow Ni(s). For the oxidation of Sn^{2+}(aq), the half-reaction is: Sn^{2+}(aq) \rightarrow Sn^{4+}(aq) + 2e^-.
Look up the standard reduction potentials (E^\circ) for each half-reaction in Appendix D. The standard reduction potential for Ni^{2+}(aq) + 2e^- \rightarrow Ni(s) is E^\circ_{Ni}. The standard reduction potential for Sn^{4+}(aq) + 2e^- \rightarrow Sn^{2+}(aq) is E^\circ_{Sn}.
Calculate the standard cell potential (E^\circ_{cell}) for the overall reaction. Use the formula: E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}. Here, the cathode is the reduction of Ni^{2+} and the anode is the oxidation of Sn^{2+}.
Determine the spontaneity of the reaction. If E^\circ_{cell} > 0, the reaction is spontaneous under standard-state conditions. If E^\circ_{cell} < 0, the reaction is non-spontaneous.
Conclude whether the reduction of Ni^{2+}(aq) by Sn^{2+}(aq) can occur under standard-state conditions based on the calculated E^\circ_{cell}.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Standard-State Conditions
Standard-state conditions refer to a set of specific conditions used to measure and compare the properties of substances. These conditions typically include a temperature of 25°C (298 K), a pressure of 1 atm, and concentrations of 1 M for solutions. Understanding these conditions is crucial for predicting the feasibility of chemical reactions, as they provide a consistent baseline for thermodynamic calculations.
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01:10
Standard Reduction Potentials
Reduction and Oxidation Reactions
Reduction and oxidation (redox) reactions involve the transfer of electrons between species. In a reduction reaction, a species gains electrons, resulting in a decrease in oxidation state, while oxidation involves the loss of electrons and an increase in oxidation state. Identifying which species is being reduced and which is being oxidized is essential for predicting the direction and spontaneity of the reaction.
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01:53Oxidation and Reduction Reactions
Electrochemical Series
The electrochemical series is a list of standard electrode potentials for various half-reactions, arranged by their ability to be reduced. It helps predict the feasibility of redox reactions by comparing the reduction potentials of the reactants. A reaction is likely to occur spontaneously if the reduction potential of the oxidizing agent is higher than that of the reducing agent, indicating a favorable electron transfer.
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02:46Electrochemical Cells
Related Practice
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The following cell reactions occur spontaneously: (b) Which of these substances (A,A+,B,B+,C,C+) is the strongest oxidizing agent? Which is the strongest reducing agent?
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What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) Oxygen gas is bubbled through an acidic solution of Cr(NO3)3.