For a reaction if `K_(p) gt K_(c)` , the forward reaction is favoured by `(T gt 15K)`

Options

A. Low pressure
B. High pressure
C. High temprature
D. Low Temprature

Explanation

To solve the question regarding the relationship between \( K_p \) and \( K_c \) and the conditions that favor the forward reaction, we can follow these steps:

### Step 1: Understand the relationship between \( K_p \) and \( K_c \)
The relationship between \( K_p \) and \( K_c \) is given by the equation:
\[ K_p = K_c (RT)^{\Delta N_g} \]
where \( R \) is the universal gas constant, \( T \) is the temperature in Kelvin, and \( \Delta N_g \) is the change in the number of moles of gas (moles of products - moles of reactants).

### Step 2: Analyze the condition \( K_p > K_c \)
Given that \( K_p > K_c \), we can infer that:
\[ (RT)^{\Delta N_g} > 1 \]
This implies that \( \Delta N_g \) must be positive, meaning that the number of gaseous moles of products is greater than that of the reactants.

### Step 3: Identify the implications of a positive \( \Delta N_g \)
Since \( \Delta N_g > 0 \), the reaction produces more gaseous moles in the forward direction. Therefore, if we want to favor the forward reaction, we should consider conditions that increase the number of moles of gas.

### Step 4: Apply Le Chatelier's Principle
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in conditions (such as pressure or temperature), the system will adjust to counteract that change and restore a new equilibrium.

### Step 5: Evaluate the effects of pressure
1. **Low Pressure**: Decreasing the pressure will shift the equilibrium towards the side with more moles of gas (the products, in this case), thus favoring the forward reaction.
2. **High Pressure**: Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas (the reactants), thus not favoring the forward reaction.

### Step 6: Evaluate the effects of temperature
Without knowing whether the reaction is exothermic or endothermic, we cannot definitively conclude how temperature changes will affect the equilibrium. Therefore, we cannot use temperature as a determining factor in this case.

### Conclusion
From the analysis, we can conclude that the forward reaction is favored by **low pressure**.