For the reaction `AB_(2)(g) rarr AB(g) + B(g)` , the initial pressure of `AB_(2)(g)` was 6 atm and at equilibrium, total pressure was found to be 8 atm at 300 K. The equilibrium constant of the reaction at 300 K is……

Explanation

To solve the problem step by step, we will analyze the reaction and the given data to find the equilibrium constant \( K_p \).

### Step 1: Write the balanced equation
The reaction is given as:
\[ AB_2(g) \rightleftharpoons AB(g) + B(g) \]

### Step 2: Set up the initial conditions
We know that the initial pressure of \( AB_2 \) is 6 atm. At the start of the reaction:
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