For the reaction $SnO_2(s) + 2H_2(g) \rightleftharpoons 2H_2O(g) + Sn(l)$,calculate $K_p$ at $900 \ K$,where the equilibrium of steam-hydrogen mixture was $45\% \ H_2$ by volume.

The equilibrium constant $K_p$ for the following reaction at $191\,^{\circ}C$ is $1.24$. What is the value of $K_c$? $B_{(s)} + \frac{3}{2}F_{2(g)} \rightleftharpoons BF_{3(g)}$

Consider the following reversible chemical reactions:
$A_{2(g)} + B_{2(g)} \overset {K_1} \leftrightarrows 2AB_{(g)} ......(1)$
$6AB_{(g)} \overset {K_2} \leftrightarrows 3A_{2(g)} + 3B_{2(g)} ......(2)$
The relation between $K_1$ and $K_2$ is:

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant at temperature $T$ is $4 \times 10^{-4}$. Find the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$.

One of the reactions that takes place in producing steel from iron ore is the reduction of iron $(II)$ oxide by carbon monoxide to give iron metal and $CO_{2}$.
$FeO(s) + CO(g) \longleftrightarrow Fe(s) + CO_{2}(g);$ $K_{p} = 0.265$ at $1050 \, K$
What are the equilibrium partial pressures of $CO$ and $CO_{2}$ at $1050 \, K$ if the initial partial pressures are: $p_{CO} = 1.4 \, atm$ and $p_{CO_{2}} = 0.80 \, atm$?

At $-20^{\circ} C$ and $1 \ atm$ pressure,a cylinder is filled with equal number of $H_2$,$I_2$ and $HI$ molecules for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$. The $K_p$ for the process is $x \times 10^{-1}$. Find the value of $x$. [Given: $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$]