A voltaic cell is constructed with two Zn²⁺-Zn electrodes. The two half-cells have [Zn²⁺] = 1.8 M and [Zn²⁺] = 1.00^.10^-2 M, respectively. (a) Which electrode is the anode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether [Zn²⁺] will increase, decrease, or stay the same as the cell operates.
We are given a concentration cell with Zn electrodes. Use the definition of a concentration cell in Section 20.6 to answer the stated questions. Use Equation [20.16] to calculate the cell emf. For a concentration cell, Q = [dilute]/[concentrated].

Question

A voltaic cell is constructed with two Zn²⁺-Zn electrodes. The two half-cells have [Zn²⁺] = 1.8 M and [Zn²⁺] = 1.00^.10^-2 M, respectively. (a) Which electrode is the anode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether [Zn²⁺] will increase, decrease, or stay the same as the cell operates.

We are given a concentration cell with Zn electrodes. Use the definition of a concentration cell in Section 20.6 to answer the stated questions. Use Equation [20.16] to calculate the cell emf. For a concentration cell, Q = [dilute]/[concentrated].

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard