If `K_(c)` is not numerically equal to `K_(p)`, how can both of the following equations be valid?
`DeltaG^(ɵ)=-2.303 RT log K_(c), DeltaG^(ɵ)=-2.303 RT log K_(p)`

Explanation

To understand how both equations \( \Delta G^{\circ} = -2.303 RT \log K_c \) and \( \Delta G^{\circ} = -2.303 RT \log K_p \) can be valid even when \( K_c \) is not numerically equal to \( K_p \), we need to analyze the definitions and relationships between these equilibrium constants.

### Step-by-Step Solution:

1. **Understanding the Definitions**:
- \( K_c \) is the equilibrium constant expressed in terms of concentrations (molarity) of the reactants and products.
- \( K_p \) is the equilibrium constant expressed in terms of partial pressures of the gaseous reactants and products.

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