For the reaction $2Ag_2O_{(s)} \rightleftharpoons 4Ag_{(s)} + O_{2(g)}$,the partial pressure of $O_2$ is given by:

For the gaseous reaction $aA + bB \rightleftharpoons cC + dD$,the relation between $K_p$ and $K_c$ is:

The equilibrium constant for the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$ is $K_{C} = 4.9 \times 10^{-2}$. The value of $K_{C}$ for the reaction $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ is:

Some solid $NH_4HS$ is placed in a flask containing $0.5 \ atm$ of $NH_3$. What would be the partial pressures of $NH_3$ and $H_2S$ when equilibrium is reached for the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$,given $K_p = 0.11$?

The value of $K_{p}$ for the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ is $3.0$ at $1000 \ K$. If initially $P_{CO_{2}} = 0.48 \ bar$ and $P_{CO} = 0 \ bar$ and pure graphite is present,calculate the equilibrium partial pressures of $CO$ and $CO_{2}$.

$4.0 \, mol$ of argon and $5.0 \, mol$ of $PCl_5$ are introduced into an evacuated flask of $100 \, L$ capacity at $610 \, K$. The system is allowed to equilibrate. At equilibrium,the total pressure of the mixture was found to be $6.0 \, atm$. The $K_p$ for the reaction is ...... [Given: $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$]