Question

What is the equilibrium constant K at 25.0 °C for an electrochemical cell when E° = +0.285 V and n = 2?(F = 96500 J/(V･mol), R = 8.314 J/(mol･K))

Answer 1

The equilibrium constant K at 25.0 °C for an electrochemical cell can be calculated using the Nernst equation.

Step-by-step explanation:

The equilibrium constant K at 25.0 °C for an electrochemical cell can be calculated using the Nernst equation. Given that E° = +0.285 V and n = 2, we can substitute these values into Equation 20.5.16 to find the value of log K:

log K = (2 * 2.05 V) / (0.0591 V)

Therefore, the equilibrium constant K can be determined by evaluating the expression on the right-hand side of the equation above.

Answer 2

The equilibrium constant, K, can be calculated using the Nernst equation and the information provided. The Nernst equation is given by Ecell = E° - (0.0591/n) * log Q. By substituting the values into the equation and solving for log K, we can find the equilibrium constant K.

Step-by-step explanation:

The equilibrium constant, K, can be calculated using the Nernst equation and the information provided. The Nernst equation is given by:

Ecell = E° - (0.0591/n) * log Q

In this case, the standard potential, E°, is given as +0.285 V and the number of electrons transferred, n, is 2. Remember that F, the Faraday constant, is 96500 J/(V·mol), and R, the ideal gas constant, is 8.314 J/(mol·K). By substituting the values into the equation and solving for log K, we can find the equilibrium constant K.