$2NO_2 \rightleftharpoons 2NO + O_2$; $K = 1.6 \times 10^{-12}$. For $NO + \frac{1}{2}O_2 \rightleftharpoons NO_2$,$K' = $

For a reaction $aA_{(g)} \rightleftharpoons bB_{(g)}$ at equilibrium,the heat of reaction at constant volume is $1500 \text{ cal}$ more than that at constant pressure. If the temperature is $27^\circ\text{C}$,then:

When one mole of $A$ and one mole of $B$ were heated in a one-litre flask at $T \ K$,$0.5 \ mole$ of $C$ was formed at equilibrium for the reaction $A + B \rightleftharpoons C + D$. The equilibrium constant,$K_C$,is:

$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$
In an equilibrium mixture,the partial pressures are
$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and
$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

For the reactions $(1)$ and $(2)$ :
$A \rightleftharpoons B + C \dots (1)$
$D \rightleftharpoons 2E \dots (2)$
Given $K_{P_1} : K_{P_2} = 9 : 1$.
If the degree of dissociation of $A$ and $D$ is the same,then the total pressure at equilibria $(1)$ and $(2)$ are in the ratio (Assume reactions are started with equal number of moles of $A$ and $D$). (in $: 1$)

At $1000\, K$ and $2\, atm$ pressure,a gaseous mixture of $CO$ and $CO_{2}$ in equilibrium with solid carbon has $84\%$ $CO_{(g)}$ by mass. Calculate $K_{p}$ for the reaction: $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$ at this temperature.