Change in molarity, temperature, volume/pressure depending on the conditions given
Explanation:
It really depends on the type of a reaction, however, we may apply general trends and see every possibility:
if we increase the concentration of products, then, according to the principle of Le Chatelier, the equilibrium will shift toward the formation of products;
if we have an endothermic reaction, increasing heat will lead a shift to the right and toward formation of products, since heat might be considered a reactant as well;
if we have an exothermic reaction, removing heat/decreasing temperature will lead to an increase in products, as we're removing one of our products, heat, and system will try to rebuild the amount of heat lost forming the other products as a result as well;
if we have gaseous substances in a reaction, an increase in pressure will shift the equilibrium to the right if we have a greater amount in moles of reactant gases compared to products, this is also known as a decrease in volume;
if we have gaseous substances in a reaction, a decrease in pressure will shift the equilibrium to the right if we have a greater amount in moles of product gases compared to reactants, this is also known as an increase in volume.
It is important to know if a resource is renewable or non-renewable because renewable resources are self-sustaining (unlike non-renewable resources). If a non-renewable resource is used too often, that resource may eventually become non-existant. This can also happen to renewable resources, but it is more difficult.
