Final answer:
Adding a solid reactant can cause the equilibrium to shift towards the right side, resulting in an increase in product concentrations.
Step-by-step explanation:
If reactant is added (increasing the denominator of the reaction quotient) or product is removed (decreasing the numerator), then Qe< Ke and the equilibrium will shift right. Note that the three different ways of inducing this stress result in three different changes in the composition of the equilibrium mixture. If H₂ is added, the right shift will consume 1₂ and produce HI as equilibrium is re-established, yielding a mixture with a greater concentrations of H₂ and HI and a lesser concentration of I₂ than was present before. If I₂ is added, the new equilibrium mixture will have greater concentrations of I₂ and HI and a lesser concentration of H₂. Finally, if HI