NEET Chemistry Chemical Equilibrium MCQs

A reaction $A(g) + B(g) \rightleftharpoons C(g)$ has a $K_c$ of 0.1 at 298 K. If initially 1 mole each of A and B are introduced into a 1L vessel, and the system is allowed to reach equilibrium, what approximate pressure change ($\Delta P$) must be applied to double the equilibrium concentration of C?

Consider the following reaction at equilibrium${N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)$if small amount of Helium gas is added to the reaction mixture at constant pressure then

Consider the following reaction at equilibrium${N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)$if small amount of Helium gas is added to the reaction mixture at constant pressure then

${K_p}/{K_c}$ for the reaction,

${\rm{CO}}\left( {\rm{g}} \right) + \frac{1}{2}{{\rm{O}}_2}\left( {\rm{g}} \right)\leftrightharpoons{\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right){\rm{is}}:$

Ammonia under a pressure of $15{\rm{ }}atm$ at $27^\circ C$ is heated to $347^\circ C$ in a closed vessel in the presence of catalyst. Under the conditions, ${\rm{N}}{{\rm{H}}_3}$ is partially decomposed according to the equation, $2{\rm{N}}{{\rm{H}}_3}\leftrightharpoons{{\rm{N}}_2} + 3{{\rm{H}}_2}$. The vessel is such that the volume remains effectively constant whereas pressure increases to $50{\rm{ }}atm$. Calculate the percentage of ${\rm{N}}{{\rm{H}}_3}$ actually decomposed

If the pressure of ${{\rm{N}}_2}/{{\rm{H}}_2}$ mixture in a closed apparatus is 100 atm and $20\%$ of the mixture then reacts, the pressure at the same temperature would be :

Final pressure is higher than initial pressure of a container filled with an ideal gas at constant temperature. What will be the value of equilibrium constant?

40% of a mixture of 0.2 mole of ${{\rm{N}}_2}$ and 0.6 mole of ${{\rm{H}}_2}$ react to give ${\rm{N}}{{\rm{H}}_3}$ according to the equation,${{\rm{N}}_2}\left( {\rm{g}} \right) + 3{{\rm{H}}_2}\left( {\rm{g}} \right)\leftrightharpoons2{\rm{N}}{{\rm{H}}_3}\left( {\rm{g}} \right)$ at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases is :

For the reaction,

${\rm{CuS}}{{\rm{O}}_4} \cdot 5{{\rm{H}}_2}{\rm{O}}\left( s \right)\leftrightharpoons{\rm{CuS}}{{\rm{O}}_4} \cdot 3{{\rm{H}}_2}{\rm{O}}\left( s \right) + 2{{\rm{H}}_2}{\rm{O}}\left( v \right)$ which one is correct representation?

For the reaction${{\rm{H}}_2}\left( {\rm{g}} \right) + {{\rm{I}}_2}\left( {\rm{g}} \right)\leftrightharpoons2{\rm{HI}}\left( {\rm{g}} \right)$, the equilibrium constants expressed in terms of concentrations ${K_c}$ and in terms of partial pressure ${K_p}$, are related as