For the reactions, $A + B + Q\;\leftrightharpoons\;C + D$  if the temperature is increased then concentration of the products will

In a gaseous reversible reaction,

${{\rm{N}}_2} + {{\rm{O}}_2}\leftrightharpoons2{\rm{NO}} + {\rm{heat}}$

If pressure is increased then the equilibrium constant would be

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 :

5 moles of ${\rm{S}}{{\rm{O}}_2}\;$ and 5 moles of ${{\rm{O}}_2}\;$ are allowed to react to forms ${\rm{S}}{{\rm{O}}_3}$ in a closed vessel. At the equilibrium stage 60% of ${\rm{S}}{{\rm{O}}_2}\;$ is used up. The total number of moles of $\;{\rm{S}}{{\rm{O}}_2}\;,{{\rm{O}}_2}\;and\;{\rm{S}}{{\rm{O}}_3}$ in the vessel now is

When pressure is applied to the equilibrium system ice r water. Which of the following phenomenon will happen?

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

For an exothermic reaction at equilibrium, increasing the temperature will:

For the reaction $A(g) \rightleftharpoons B(g) + C(g)$, if the total pressure at equilibrium is P, and the partial pressure of A is $P_A$, the equilibrium constant $K_p$ is:

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?

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?

What is the effect of having the pressure by doubling the volume on the following system at $500^\circ C$?

${{\rm{H}}_2}\left( {\rm{g}} \right) + {{\rm{I}}_2}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{HI}}\left( {\rm{g}} \right)$