Final answer:
Increasing the total pressure on the chemical reaction H2(g) + CO2(g) ⇔ H2O(g) + CO(g) does not shift the equilibrium since the number of gas moles on both sides is the same. Le Châtelier's Principle indicates that equilibrium shifts occur to counteract pressure changes, but in this case, it remains unaffected.
Step-by-step explanation:
The question concerns the effect of increasing the total pressure on the equilibrium of the chemical reaction: H2(g) + CO2(g) ⇌ H2O(g) + CO(g), ΔHo = +41.2 kJ/mol. According to Le Châtelier's Principle, if the pressure is increased, the equilibrium will shift toward the side with fewer moles of gas to minimize the change. In this case, since the number of gas moles is the same on both sides of the equation, pressure increase will have no effect on the position of the equilibrium. However, because the reaction is endothermic (ΔHo is positive), increasing temperature would cause the reaction to shift towards the products. Enthalpy and entropy changes in other reactions, such as the formation of CO2 or NO2, provide context but are not directly applicable to this equilibrium scenario.