For the reaction
`2SO_(2)(g)+O_(2)(g)=2SO_(3)(g)`
`deltaH=-57.2kJmol^(-1)` and `K_(C)=1.7xx10^(16)` ltbr. Which of the following statements is INCORRECT?

Options

A. The equilibrium constant decreases as the temperature increases
B. The addition of inert gas at constant volume will not affect the equilibrium constant
C. The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
D. The equilibrium will shift in forward direction as the pressure increases

Explanation

To determine which statement is INCORRECT regarding the reaction

\[ 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) \]

with \(\Delta H = -57.2 \, \text{kJ/mol}\) and \(K_C = 1.7 \times 10^{16}\), we will analyze each statement one by one.

### Step 1: Analyze the first statement
**Statement 1:** "Equilibrium constant decreases as the temperature increases."

- Since the reaction is exothermic (as indicated by the negative \(\Delta H\)), an increase in temperature will shift the equilibrium to the left (towards the reactants) according to Le Chatelier's principle. This results in a decrease in the equilibrium constant \(K_C\).
- Therefore, this statement is **CORRECT**.

### Step 2: Analyze the second statement
**Statement 2:** "Addition of inert gas at constant volume will not affect the equilibrium constant."

- When an inert gas is added at constant volume, it does not change the partial pressures or concentrations of the reactants and products. Thus, the equilibrium constant \(K_C\) remains unchanged.
- Therefore, this statement is **CORRECT**.

### Step 3: Analyze the third statement
**Statement 3:** "Equilibrium constant is large suggestive of reaction going to completion and catalysis required."

- A large \(K_C\) indicates that at equilibrium, the concentration of products is much greater than that of reactants, suggesting that the reaction favors the formation of products. However, this does not imply that the reaction goes to completion; it only indicates a strong tendency to form products.
- Additionally, a catalyst speeds up the rate of reaching equilibrium but does not affect the value of \(K_C\).
- Therefore, this statement is **INCORRECT**.

### Step 4: Analyze the fourth statement
**Statement 4:** "The equilibrium will shift in the forward direction as the pressure increases."

- To analyze this, we calculate \(\Delta N_g\):
\[ \Delta N_g = N_p - N_r = 2 - (2 + 1) = -1 \]
- Since \(\Delta N_g\) is negative, increasing pressure will shift the equilibrium towards the side with fewer moles of gas, which is the product side (forward direction).
- Therefore, this statement is **CORRECT**.

### Conclusion
The INCORRECT statement is **Statement 3**: "Equilibrium constant is large suggestive of reaction going to completion and catalysis required."

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