When $1 \ mol$ of $H_2$ and $1 \ mol$ of $N_2$ are enclosed in a $5 \ L$ vessel and the reaction is allowed to attain equilibrium,it is found that at equilibrium there is $x \ mol$ of $H_2$. The number of moles of $NH_3$ would be

At $783 \, K$ in the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the molar concentrations $(mol \, L^{-1})$ of $H_2, I_2$ and $HI$ at some instant of time are $0.1, 0.2$ and $0.4$,respectively. If the equilibrium constant is $46$ at the same temperature,then as the reaction proceeds:

Write a relation between $\Delta G$ and $Q$ and define the meaning of each term and answer the following:
$(a)$ Why a reaction proceeds forward when $Q < K$ and no net reaction occurs when $Q = K$.
$(b)$ Explain the effect of increase in pressure in terms of reaction quotient $Q$.
For the reaction: $CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_{2}O_{(g)}$

At $T$ $(K)$,the equilibrium constant for the reaction $H_{2(g)} + Br_{2(g)} \rightleftharpoons 2 HBr_{(g)}$ is $1.6 \times 10^5$. If $10 \ bar$ of $HBr$ is introduced into a sealed vessel at $T$ $(K)$,the equilibrium pressure of $HBr$ (in $bar$) is approximately

The value of $K_{c} = 4.24$ at $800 \, K$ for the reaction,
$CO_{(g)} + H_{2}O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$
Calculate equilibrium concentrations of $CO_{2}$,$H_{2}$,$CO$ and $H_{2}O$ at $800 \, K$,if only $CO$ and $H_{2}O$ are present initially at concentrations of $0.10 \, M$ each.

At a certain temperature,the equilibrium constant $K_c$ is $0.25$ for the reaction:
$A_{2(g)} + B_{2(g)} \rightleftharpoons C_{2(g)} + D_{2(g)}$
If we take $1 \ mol$ of each of the four gases in a $10 \ L$ container,what would be the equilibrium concentration of $A_{2(g)}$ (in $M$)?