In the Nernst equation, we substitute
`(2.303RT)/F=0.0591`
where,

Options

A. R = 8.314 J, T = 273 K and F = 96500 C
B. R = 0.0821 L. atm, T = 298 K and F = 96500 C
C. R = 8.314 J, T = 298 K and F = 96500 C
D. R = 2.0 cal, T = 298 K and F = 1 C

Answer

To solve the question regarding the Nernst equation and the substitution of \( \frac{2.303RT}{F} = 0.0591 \), we need to identify the units of \( R \), \( F \), and \( T \).

### Step-by-Step Solution:

1. **Identify the Constants**:
- \( R \) is the universal gas constant.
- \( F \) is Faraday's constant.
- \( T \) is the temperature in Kelvin.

2. **Units of Faraday's Constant (F)**:
- Faraday's constant \( F \) is defined as the charge per mole of electrons.
- The unit of \( F \) is Coulombs per mole (C/mol).
- The value of \( F \) is approximately \( 96500 \, C/mol \).

3. **Units of Temperature (T)**:
- The temperature \( T \) is measured in Kelvin (K).
- For this equation, we typically use standard room temperature, which is \( 298 \, K \).

4. **Units of the Gas Constant (R)**:
- The universal gas constant \( R \) can be expressed in multiple units. However, for this context, we will use the value in Joules per mole per Kelvin (J/(mol·K)).
- The value of \( R \) is approximately \( 8.314 \, J/(mol·K) \).

5. **Substituting Values into the Nernst Equation**:
- The Nernst equation involves the term \( \frac{2.303RT}{F} \).
- When substituting the values into the equation:
- \( R = 8.314 \, J/(mol·K) \)
- \( T = 298 \, K \)
- \( F = 96500 \, C/mol \)

6. **Calculating \( \frac{2.303RT}{F} \)**:
- Substitute the values into the equation:
\[ \frac{2.303 \times 8.314 \times 298}{96500} \]
- Performing the calculation gives approximately \( 0.0591 \).

### Conclusion:
Thus, we confirm that \( \frac{2.303RT}{F} = 0.0591 \) holds true with the specified units for \( R \), \( F \), and \( T \).