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:

$K_{c}$ for the reaction,$A_{2(g)} \rightleftarrows B_{2(g)}$ is $99.0$. In a $1 \ L$ closed flask,two moles of $B_{2(g)}$ are heated to $T(K)$. What is the concentration of $B_{2(g)}$ (in $mol \ L^{-1}$) at equilibrium?

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

For the reaction $A_{(g)} \rightleftharpoons B_{(g)}$ at $495 \ K$,$\Delta_{r}G^{\circ} = -9.478 \ kJ \ mol^{-1}$. If we start the reaction in a closed container at $495 \ K$ with $22 \ mmol$ of $A$,the amount of $B$ in the equilibrium mixture is $x \ mmol$. Find $x$ (Round off to the nearest integer). $[R = 8.314 \ J \ mol^{-1} \ K^{-1}; \ln 10 = 2.303]$

In which of the following plots,an endothermic reaction is correctly represented?

Consider the following reaction in a $1 \ L$ closed vessel: $N_2 + 3H_2 \rightleftharpoons 2NH_3$. If all the species $N_2, H_2$ and $NH_3$ are $1 \ mol$ each at the beginning of the reaction and equilibrium is attained when unreacted $N_2$ is $0.7 \ mol$,what is the value of the equilibrium constant?