At $298 \, K$,for which of the following reactions will the value of $\frac{K_p}{K_c}$ be maximum and minimum,respectively?
$(a) N_2O_4 \rightleftharpoons 2NO_2$
$(b) 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$(c) X + Y \rightleftharpoons 4Z$
$(d) A + 3B \rightleftharpoons 7C$

For the following gaseous reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$,the equilibrium constant relationship is:

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,what is the relationship between $K_p$ and $K_c$?

Equilibrium constants for the following reactions at $1200 \ K$ are given:
$2 \ H_2O_{(g)} \rightleftharpoons 2 \ H_{2(g)} + O_{2(g)}$
$K_1 = 6.4 \times 10^{-8}$
$2 \ CO_{2(g)} \rightleftharpoons 2 \ CO_{(g)} + O_{2(g)}$
$K_2 = 1.6 \times 10^{-6}$
The equilibrium constant for the reaction: $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$
at $1200 \ K$ will be

What is the value of the equilibrium constant $K_p$ for the reaction ${H_2O_{(l)}} \rightleftharpoons {H_2O_{(g)}}$ at $60^{\circ}C$? (The vapor pressure of water at $60^{\circ}C$ is $0.185 \ bar$.)

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: