Answer: the only stress that would increase the yield of products (shift right) is decreasing the temperature (e) or increasing the volume (c).
Step-by-step explanation:
Due to the endothermic nature of the given reaction in the forward direction, there will be a net absorption of heat from the system's surroundings during the course of the forward reaction progression. Reducing the temperature would facilitate the progress of the endothermic course and induce a rightward shift in the reaction.
Moreover, due to a reduction in the number of gaseous moles present on the product side, an amplification in volume would lead to a decline in the overall concentration of the produced species. Consequently, the reaction equilibrium would pivot towards the right-hand side.
Alternatively, raising the pressure would promote the progression of the reaction toward the side with a lower number of gaseous entities. Consequently, the reaction would experience a leftward shift, thereby opposing the intended direction.
Reciprocally, a reduction in the concentration of reactants would induce a shift of the reaction towards the left direction. This phenomenon arises from the decrease in the quantity of reactive particles available to yield collisions and reactions, therefore culminating in a diminished progress rate of the forward reaction.