Question

which change(s) will shift this exothermic reaction to the right? select all that apply. x(g) 2 y(g) xy2(g) group of answer choices decreasing the partial pressure of y heating the container decreasing the partial pressure of xy2 adding a catalyst adding argon gas while holding the container volume constant

Answer 1

Decreasing the volume increases pressure and shifts the equilibrium to the right. Increasing the temperature shifts the equilibrium to the left. Raising the temperature shifts the equilibrium to the right.

Step-by-step explanation:

Decreasing the volume leads to an increase in pressure which will cause the equilibrium to shift towards the side with fewer moles. In this reaction, there are three moles on the reactant side and two moles on the product side, so the new equilibrium will shift towards the products (to the right).

Increasing the temperature of the reaction increases the internal energy of the system. Thus, increasing the temperature has the effect of increasing the amount of one of the products of this reaction. The reaction shifts to the left to relieve the stress, and there is an increase in the concentration of H₂ and I₂ and a reduction in the concentration of HI. Lowering the temperature of this system reduces the amount of energy present, favors the production of heat, and favors the formation of hydrogen iodide.

Raising the temperature of the system is akin to increasing the amount of a reactant, and so the equilibrium will shift to the right. Lowering the system temperature will likewise cause the equilibrium to shift left. For exothermic processes, heat is viewed as a product of the reaction and so the opposite temperature dependence is observed.