Question

Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0285 M, the pH of the H+ cell is 2.500, and the pressure for H2 is held constant at 1 atm. The temperature is held constant at 55°C

Answer 1

To calculate the potential for the electrochemical cell, use the Nernst equation and the given concentrations of Ag+ and H+. Plug in the values to calculate the cell potential.

Step-by-step explanation:

To calculate the potential for the electrochemical cell, we can use the Nernst equation. The Nernst equation is given by E = E° - (0.0592/n) log(Q), where E is the cell potential, E° is the standard cell potential, n is the number of electrons transferred, and Q is the reaction quotient. In this case, the anode is the compartment with Ag+, and the cathode is the compartment with H+. The half-reactions can be written as follows:

Ag+ (aq) + e¯ → Ag(s)

2H+ (aq) + 2e¯ → H2(g)

The standard potential for the Ag+ → Ag half-reaction is known to be 0.799 V, and the standard potential for the H+ → H2 half-reaction is 0 V. Plugging in the given concentrations and the Nernst equation, we can calculate the potential for the cell.