If `Delta G^(@)gt 0` for a reaction then :

Options

A. `K_(P) gt 1`
B. `K_(P) lt 1`
C. The products predominate in the equilibrium mixture
D. None

Answer

To solve the question "If ΔG° > 0 for a reaction then:", we will analyze the relationship between the Gibbs free energy change (ΔG°) and the equilibrium constant (Kp) for a reaction.

### Step-by-Step Solution:

1. **Understand the Gibbs Free Energy Change**:
- The Gibbs free energy change (ΔG°) is a thermodynamic quantity that indicates the spontaneity of a reaction. If ΔG° is positive, the reaction is non-spontaneous under standard conditions.

2. **Relationship Between ΔG° and Kp**:
- The relationship between ΔG° and the equilibrium constant (Kp) is given by the equation:
\[ ΔG° = -RT \ln Kp \]
- Where R is the universal gas constant and T is the temperature in Kelvin.

3. **Analyzing the Equation**:
- If ΔG° > 0, then:
\[ -RT \ln Kp > 0 \]
- This implies that:
\[ \ln Kp < 0 \]
- Therefore, Kp must be less than 1 because the natural logarithm of a number less than 1 is negative.

4. **Conclusion**:
- Since Kp < 1, this indicates that at equilibrium, the reactants predominate over the products. Hence, the correct answer to the question is that Kp is less than 1.

### Final Answer:
- Kp is less than 1.