An electrochemical cell is constructed with a zinc metal anode in contact with a 0.052 M solution of zinc nitrate and a silver cathode in contact with a 0.0042 M solution of silver (I) nitrate. What is the value of Q to use in the Nernst equation for this cell

Question

Chemistry

Miles Watson

20 August, 13:15

An electrochemical cell is constructed with a zinc metal anode in contact with a 0.052 M solution of zinc nitrate and a silver cathode in contact with a 0.0042 M solution of silver (I) nitrate. What is the value of Q to use in the Nernst equation for this cell

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Answers (1)

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Uriel Morgan · Answer 1

Q = 12.38

Explanation:

The Nernst equation is given as; Ecell = E°cell - (2.303RT/nF) log Q; where Q is the reaction quotient.

The reaction quotient, Q in a reaction, is the product of the concentrations of the products divided by the product of the concentrations of the reactants.

In an electrochemical cell, Q is the ratio of the concentration of the electrolyte at the anode to that of the electrolyte at the cathode.

Q = [anode]/[cathode]

therefore, Q = 0.052/0.0042 = 12.38