An inert gas is added to the following equilibrium,
`A(s)+2B(g)hArr3C(g)`
at constant pressure. The equilibrium

Options

A. is not affected
B. shifts to right
C. shifts to left
D. may shift right and left both

Answer

To solve the question regarding the effect of adding an inert gas to the equilibrium reaction \( A(s) + 2B(g) \rightleftharpoons 3C(g) \) at constant pressure, we can follow these steps:

### Step 1: Understand the Reaction
The reaction involves a solid \( A \) and two gases \( B \) and \( C \). The equilibrium is established between the solid and the gaseous products.

### Step 2: Identify the Role of Inert Gas
An inert gas does not react with the components of the equilibrium. When added to the system, it increases the total pressure but does not change the partial pressures of the reactants or products involved in the equilibrium.

### Step 3: Consider the Effect on Equilibrium
According to Le Chatelier's Principle, if an inert gas is added at constant volume, the equilibrium will shift towards the side with fewer moles of gas. However, since we are adding the inert gas at constant pressure, the volume of the system will increase, and the partial pressures of the gases \( B \) and \( C \) will remain unchanged.

### Step 4: Conclusion
Since the addition of an inert gas at constant pressure does not affect the partial pressures of the reactants and products, the position of equilibrium will not shift. Therefore, the equilibrium remains unchanged.

### Final Answer
The equilibrium will not shift when an inert gas is added at constant pressure.

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