For the homogeneous gaseous equilibrium , what will happen if the volume of the reaction container i — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

Halving the volume instantly doubles the pressure and concentrations of all species. The system has 5 moles of gaseous reactants and 4 moles of gaseous products ($\Delta n_g = -1$). To relieve the increased pressure, the equilibrium shifts forward (towards fewer moles). Even after the shift, the volume reduction dominates, making final concentrations and total pressure higher than the initial state. $K_c$ remains constant as temperature is unchanged.