The vapour density of completely dissociated ${\rm{N}}{{\rm{H}}_4}{\rm{Cl}}$ would be:

In which of the following reactions, the concentration of product is higher than the concentration of reactant at equilibrium? $\left( {K = \;\;{\rm{equilibrium}}\;{\rm{ constant}}} \right)$

A system at equilibrium is described by the reaction $A(g) + B(g) \rightleftharpoons C(g)$ with $K_c = 10$ at 298 K. If the initial concentrations are [A] = 0.1 M, [B] = 0.2 M, and [C] = 0.3 M, which direction will the reaction proceed to reach equilibrium?

A chemical reaction $A\,\,\leftrightharpoons\,\,B$ is said to be at equilibrium when:

1 mole of ${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)$ at 300 K is kept in a closed container under 1 atm. It is heated to 600 K when 20% by mass of${{\rm{N}}_2}{{\rm{O}}_4}\left( {\rm{g}} \right)$ decomposes to ${\rm{N}}{{\rm{O}}_2}\left( {\rm{g}} \right)$. The resultant pressure is

A reversible chemical reaction is having two reactants, in equilibrium. If the concentration of the reactants are doubled then the equilibrium constant will

For the reversible reactions. $CaC{O_{3\left( S \right)}}Ca{O_{\left( s \right)}} + C{O_{2\left( g \right)}}$, Which of the following does not affect the equilibrium state ?

A mixture of $0.3{\rm{ }}\;mole$ of ${{\rm{H}}_2}$ and $0.3{\rm{ }}\;mole$ of ${{\rm{I}}_2}$ is allowed to react in a 10 L evacuated flask at $500^\circ C$. The reaction is ${{\rm{H}}_2} + {{\rm{I}}_2}\leftrightharpoons2{\rm{HI}},$ the $K$ is found to be 64. The amount of unreacted ${{\rm{I}}_2}$ at equilibrium is

The chemical equilibrium of a reversible reaction is not influenced by

For the Haber’s process for the formation of ${\rm{N}}{{\rm{H}}_3}$ at ${\rm{298}}\;{\rm{K}}$ is :${{\rm{N}}_2} + 3{{\rm{H}}_2}\;\leftrightharpoons2{\rm{N}}{{\rm{H}}_3};\;\;\Delta H = - 460\;\;{\rm{kJ}}$Which of the following is correct?

For the reaction $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$ at $250^\circ C$, the equilibrium partial pressures are $P_{PCl_5} = 0.5\,\mathrm{atm}$, $P_{PCl_3} = 0.15\,\mathrm{atm}$, and $P_{Cl_2} = 0.15\,\mathrm{atm}$. Calculate $\Delta G^{\circ}$ for the reaction. $(R = 8.314\,\mathrm{J}\,\mathrm{mol}^{-1}\mathrm{K}^{-1})$