For the reaction $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$,the partial pressures of $CO$ and $CO_2$ at equilibrium are $2.0 \ atm$ and $4.0 \ atm$ respectively. The value of $K_p$ for the reaction is:

For which of the following reactions does the equilibrium constant depend on the units of concentration?

$(1) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} \ ; \ K_1$
$(2) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)} \ ; \ K_2$
$(3) \ H_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons H_2O_{(g)} \ ; \ K_3$
The equation for the equilibrium constant of the reaction
$2NH_{3(g)} + \frac{5}{2}O_{2(g)} \rightleftharpoons 2NO_{(g)} + 3H_2O_{(g)}$
$(K_4)$ in terms of $K_1$,$K_2$,and $K_3$ is

For the reaction $CO(g) + Cl_2(g) \rightleftharpoons COCl_2(g)$,the value of $\frac{K_P}{K_C}$ is equal to which of the following?

For a reversible reaction $A \rightleftharpoons B$,the equilibrium concentration of $B$,denoted as $[B]_e$,is given by which expression?

For which of the following reactions will ${K_p} > {K_c}$?