The equilibrium constant $(K_P)$ for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ at $1000 \ K$ is $3.5$. The partial pressure of oxygen gas to give equal mole of $SO_2$ and $SO_3$ is $... \ atm$.

For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $NO_{(g)} \rightleftharpoons 1/2N_{2(g)} + 1/2O_{2(g)}$,the equilibrium constants are $K_1$ and $K_2$ respectively. What is the relationship between $K_1$ and $K_2$?

The equilibrium constant for the reversible reaction,$N_2 + 3H_2 \rightleftharpoons 2NH_3$ is $K$ and for the reaction $\frac{1}{2}N_2 + \frac{3}{2}H_2 \rightleftharpoons NH_3$ the equilibrium constant is $K'$. $K$ and $K'$ will be related as

For the chemical equilibrium,$CaCO_{3_{(s)}} \rightleftharpoons CaO_{(s)} + CO_{2_{(g)}}$,$\Delta H_{r}^{\circ}$ can be determined from which one of the following plots?

The value of $K_{C}$ for the equilibrium reaction: $CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ at $T \ K$ is $0.036$. If the equilibrium concentration of $CO_{2(g)}$ is $0.004 \ M$,the concentration of $CO_{(g)}$ in $mol \ L^{-1}$ is: