One mole of $N_2O_{4(g)}$ at $300 \ K$ is kept in a closed container under $1 \ atm$ pressure. It is heated to $600 \ K$ when $20 \%$ of $N_2O_{4(g)}$ decomposes to $NO_{2(g)}$. The resultant pressure at $600 \ K$ is $..... \ atm$.

Assign $A, B, C, D$ from the given type of reaction.
$PbCl_2 \downarrow + H_2SO_4 \rightleftharpoons PbSO_4 \downarrow + 2HCl$

In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:
$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

In the reaction $A + 2B \rightleftharpoons 2C$,if $2$ moles of $A$,$3.0$ moles of $B$ and $2.0$ moles of $C$ are placed in a $2.0 \ L$ flask and the equilibrium concentration of $C$ is $0.5 \ mol/L$. The equilibrium constant $K_c$ for the reaction is:

In a $0.25 \ L$ tube,$4 \ mol$ of $NO$ undergoes dissociation. If the degree of dissociation is $10\%$,then the value of $K_c$ for the reaction $2NO \rightleftharpoons N_2 + O_2$ will be:

At $1000 \ K$,the equilibrium constant for the reaction $CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$ is $0.53$. In a one litre vessel,at equilibrium the mixture contains $0.25 \ mole$ of $CO$,$0.5 \ mole$ of $CO_2$,$0.6 \ mole$ of $H_2$ and $x \ moles$ of $H_2O$. The value of $x$ is