Question

At $T(K)$ consider the following equilibrium reaction \[ HgO(s) \rightleftharpoons Hg(g)+\frac{1}{2}O_2(g) \] The correct relation between $K_p$ and $P_{Total}(P_T)$ is}

• A. $K_p = \frac{2}{3^{1/2}}.P_T^{1/2}$
• B. $K_p = \frac{2}{3^{3/2}}.P_T^{3/2}$
• C. $K_p = \frac{2}{3^{2/3}}.P_T^{2/3}$
• D. $K_p = \frac{1}{3^{2/3}}.P_T$ \bigskip

Hint:

For gaseous equilibrium problems:
• Find mole fractions.
• Convert to partial pressures using \[ P_i=y_iP_T \]
• Substitute into the expression of \(K_p\). Always omit solids and pure liquids from equilibrium constant expressions.

Answer 1

The Correct Option is B