For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,if the total pressure in the reaction vessel at $105 \ ^\circ C$ is $1.12 \ atm$,then the $K_p$ for this equilibrium will be .........

For the reaction: $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$,$K_P = 2 \times 10^{12}$ at $27^{\circ} C$ and $1 \ atm$ pressure. The $K_C$ for the same reaction is $......... \times 10^{13}$. (Nearest integer)
(Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$,which of the following relations is correct?

For the reaction $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$,the partial pressure of $CO_2$ and $CO$ at equilibrium are $4 \ atm$ and $8 \ atm$ respectively. $K_p$ for the reaction is

For the following reaction in gaseous phase $CO + 1/2 O_2 \to CO_2$,the ratio $K_p/K_c$ is:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be: