Question

7. In the Nernst equation the value of 2.303 RT/nF is equal to 0.0592 when
a) R in calories, n= 1 and T = 298 b) R in calories, n=2andT=25
c) R in joule, n = 1 and T = 298 d) R in joule, n=land T=25​

Answer 1

option c is correct . . . .

Answer 2

The answer is C; R in joule, n=1, and T=298K

Explanation:

The Nernst equation is often used to calculate the cell potential of an electrochemical cell at any given temperature, pressure, and reactant concentration. The equation was introduced by a German chemist Walther Hermann Nernst.

              Ecell = E° – [RT/nF] ln Q

Nernst Equation at 25°C

For measurements carried out 298K, the Nernst equation can be expressed as follows.

E = E° – 0.0592/n log₁₀ Q

Therefore, as per the Nernst equation, the overall potential of an electrochemical cell is dependent on the reaction quotient.