The standard Gibbs energy change at $300 \, K$ for the reaction $2A \rightleftharpoons B + C$ is $2494.2 \, J$. At a given time,the composition of the reaction mixture is $[A] = 1/2, [B] = 2$ and $[C] = 1/2$. The reaction proceeds in the:

When $5 \ mol$ of $SO_2$ and $5 \ mol$ of $O_2$ are reacted,$60\%$ of $SO_2$ is consumed at equilibrium. If the total pressure of the equilibrium mixture is $1 \ atm$,then the partial pressure of $O_2$ will be ...... $atm$.

For the following reactions,equilibrium constants are given:
$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$
$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$
The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is:

For the reaction $CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_{2}O_{(g)}$ with $\Delta H = -170.8 \ kJ \ mol^{-1}$,which of the following statements is incorrect?

The distribution law is applied for the distribution of a solute between which of the following pairs of solvents?

$K_{c}$ for the following reaction is $99.0$: $A_{2(g)} \rightleftharpoons B_{2(g)}$. In a $1 \ L$ flask,$2 \ moles$ of $A_{2}$ were heated to $T(K)$ and equilibrium was reached. The concentrations at equilibrium of $A_{2}$ and $B_{2}$ are $C_{1}(A_{2})$ and $C_{2}(B_{2})$ respectively. Now,$1 \ mole$ of $A_{2}$ was added to the flask and heated to $T(K)$ to establish equilibrium again. The concentrations of $A_{2}$ and $B_{2}$ are $C_{3}(A_{2})$ and $C_{4}(B_{2})$ respectively. What is the value of $C_{3}(A_{2})$ in $mol \ L^{-1}$?