Question

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

Answer 1

The value of Q for the zinc and silver electrochemical cell is the ratio of the concentrations of Zn²+ and Ag²+, which is 0.052 M (for Zn²+) divided by 0.0042 M (for Ag²+), resulting in a value of approximately 12.38.

Step-by-step explanation:

The value of Q in the Nernst equation for an electrochemical cell, such as the one constructed with a zinc metal anode and a silver cathode, can be determined using the reaction quotient expression Q = [Zn²+]/[Cu²+]. In this case, since we have a zinc 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, the reaction quotient would be Q = [Zn²+]/[Ag²+]. Substituting the given concentrations, we have Q = 0.052 M / 0.0042 M which can be calculated to find the numerical value to be used in the Nernst equation.
To find the exact value of Q for this electrochemical cell, we perform the calculation: Q = 0.052 / 0.0042, which equals approximately 12.38. This value of Q is what you would use in the Nernst equation to calculate the cell potential at these given concentrations of zinc and silver ions.

Answer 2

Q = 12.38

Step-by-step 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