At $298 \ K$,the value of $K_p$ for $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ is $0.113 \ atm$. The partial pressure of $N_2O_4$ at equilibrium is $0.2 \ atm$. What is the partial pressure (in $atm$) of $NO_2$ at equilibrium?

For the reaction $CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$,$\frac{K_p}{K_c}$ is equal to

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_p = 41$ at $400 \ K$. Calculate $K_c$ for the following reactions at $400 \ K$:
$(a)$ $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$
$(b)$ $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$
$(c)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$

For which of the following reactions will the value of $\Delta n = \sum n_p - \sum n_r$ be positive? $(1)$ $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ $(2)$ $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ $(3)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

$5.1 \ g$ $NH_4SH$ is introduced in a $3.0 \ L$ evacuated flask at $327 \ ^\circ C$. $30\%$ of the solid $NH_4SH$ decomposes into $NH_3$ and $H_2S$ gases. The $K_p$ of the reaction at $327 \ ^\circ C$ is ($R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$,molar mass of $S = 32 \ g \ mol^{-1}$,molar mass of $N = 14 \ g \ mol^{-1}$)

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the value of $K_p$ at $800 \ ^oC$ is $1.16 \ atm$. If $1 \ mol$ of $CaCO_{3(s)}$ is taken in a $1 \ L$ container to start the reaction,what will be the partial pressure of $CO_2$ at equilibrium in $atm$?