Final answer:
To increase the products of an endothermic reaction with a positive ΔH, the temperature should be increased. This causes the equilibrium to shift towards the products as the system counteracts the added heat by favoring the reaction that absorbs it.
Step-by-step explanation:
Temperature's Effect on Chemical Equilibrium
The effect of temperature on chemical equilibrium is a critical concept in thermodynamics. When dealing with a chemical reaction with a positive enthalpy change (ΔH), like the endothermic reaction we are considering which has a ΔH of 57 kJ, we need to think about temperature as a component of the reaction. Since an endothermic reaction absorbs heat, increasing the temperature adds more energy to the system, effectively acting as if we are adding more reactants. Hence, to increase the products, we need to increase the temperature. Doing so shifts the equilibrium towards the products. Conversely, lowering the temperature would shift the equilibrium back towards the reactants. This understanding is based on Le Chatelier's Principle, which describes how a system at equilibrium responds to changes in concentration, temperature, volume, or pressure.
If the goal is to drive the reaction towards more products and we know that the reaction absorbs heat (as indicated by the positive ΔH), we must raise the temperature. This is akin to adding a reactant, which causes the equilibrium to shift towards the products. This shift to produce more products occurs because the system is trying to counteract the added heat (reactant) by consuming it, hence favoring the endothermic process that absorbs heat.