At `1065^(0)C, K_(p)`= 0.118 atm for the reaction `2H_(2)S(g) Leftrightarrow 2H_(2) (g)+S_(2)(g)` The enthalpy of the reaction is 177.3 kJ/mol. Calculate the given equilibrium constant at `1200^(@)C` Given R=8.314 J

Explanation

To solve the problem of calculating the equilibrium constant \( K_p \) at \( 1200^{\circ}C \) given the equilibrium constant at \( 1065^{\circ}C \) and the enthalpy change of the reaction, we will use the Van't Hoff equation. Here’s a step-by-step solution:

### Step 1: Convert the Temperatures to Kelvin
The first step is to convert the temperatures from Celsius to Kelvin.

- For \( T_1 = 1065^{\circ}C \):
\[
T_1 = 1065 + 273 = 1338 \, K
...