The incorrect statement among the following for this reaction is

Options

A. decrease in total pressure will result in the formation of more moles of gaseous X.
B. At the start of the reaction, dissociation of gaseous `X_2` takes place spontaneouly.
C. `beta_("eqb")=0.7`
D. `K_(C) lt 1`

Answer

To solve the question regarding the incorrect statement for the given reaction, we will analyze each option step by step.

### Step 1: Understand the Reaction and Equilibrium
The question revolves around a chemical reaction that reaches equilibrium. In equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

### Step 2: Analyze the Options
1. **Option 1**: "Decrease in total pressure will result in the formation of more moles of gaseous products."
- According to Le Chatelier's principle, if the pressure is decreased, the equilibrium will shift towards the side with more moles of gas. This statement is correct.

2. **Option 2**: "At the start of the reaction, dissociation of gaseous reactants takes place simultaneously."
- This statement indicates that the reaction can proceed in both directions initially. This is also a correct statement.

3. **Option 3**: "When you calculate the value of Kp, you will get 8 beta equivalent square upon 4 minus beta equivalent square, and this value will be more than 1."
- This statement suggests a specific calculation of Kp and claims that it is greater than 1. However, if the conditions of the reaction lead to a scenario where Kp is less than 1, this statement is incorrect.

4. **Option 4**: "Kc should be less than 1 because we know that delta G is equal to -RT ln K, and K must be less than 1 to make delta G negative."
- This statement is correct as it relates the Gibbs free energy change to the equilibrium constant K. If K is less than 1, it indicates that the reaction favors the reactants at equilibrium.

### Step 3: Identify the Incorrect Statement
From the analysis:
- Options 1, 2, and 4 are correct.
- Option 3 is incorrect because it claims that Kp is greater than 1, which contradicts the given conditions.

### Conclusion
The incorrect statement among the options is **Option 3**.

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