Consider the equilibrium reaction: CO (g) + H2 (g) ⇌ C (s) + H2O (g), ΔHr = –131.3 kJ mol–1 Making use of Le Chatelier’s principle, identify which of the following will happen if the temperature of the system is increased.

Question

Consider the equilibrium reaction: CO (g) + H2 (g) ⇌  C (s) + H2O (g), ΔHr = –131.3 kJ mol–1 Making use of Le Chatelier’s principle, identify which of the following will happen if the temperature of the system is increased.

BlackTom AI · Accepted Answer

To tackle this, I’ll review how temperature changes affect an exothermic reaction in equilibrium using Le Chatelier’s principle.
Option a: 'The reaction equilibrium is unchanged.' This is incorrect because changing temperature for a system at equilibrium does perturb the position of equilibrium unless the temperature change somehow has no effect on the Gibbs free energy landscape, which is not the case here since ΔH is nonzero. In practice, temperature is a driving force for shifting toward the direction that absorbs or releases heat.
Option b: 'The reaction will move towards reactants.' This aligns with Le Chatelier’s principle for an exothermic reaction (ΔH < 0). Increasing temperature adds heat to the system; the system counteracts this by shifting toward the side that consumes heat — the endothermic direction. In this reaction, the endothermic direction is the reverse process (toward CO and H2) forming C(s) and H2O is exothermic, so the shift is toward the reactants. Therefore, this option correctly describes the expected shift.
Option c: 'The reaction moves, but it cannot be determined in which direction.' This is not accurate here because the sign of ΔH gives a clear predictor: an increase in temperature pushes the equilibrium toward the endothermic direction. Thus, the direction can be determined.
Option d: 'The reaction will move towards products.' This would be expected if the temperature were decreased for an exothermic reaction or increased for an endothermic reaction. Since the temperature is increased in an exothermic process, this option contradicts the established behavior and is therefore incorrect.
Summing up, the temperature rise drives the system to lessen the added heat, i.e., toward the endothermic direction, which corresponds to the reactants in this reaction. The other choices fail because they conflict with the thermodynamic sign of ΔH and the basic predictive use of Le Chatelier’s principle.

Consider the equilibrium reaction: CO (g) + H2 (g) ⇌ C (s) + H2O (g), ΔHr = –131.3 kJ mol–1 Making use of Le Chatelier’s principle, identify which of the following will happen if the temperature of the system is increased.

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Consider the equilibrium reaction: CO (g) + H2 (g) ⇌ C (s) + H2O (g), ΔHr = –131.3 kJ mol–1 Making use of Le Chatelier’s principle, identify which of the following will happen if the temperature of the system is increased.

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类似问题

Methanol is manufactured by the following exothermic reaction. CO (g) + 2H2 (g) ⇌ CH3OH (g) Which pair of changes will favour the forward reaction?[Fill in the blank]

Chemical equilibrium is the state where chemical reactions are in balance and no longer occurring.

For the reaction N2(g) + 3 H2(g) 2 NH3(g) Kc = 0.0600 at a certain temperature. In an equilibrium mixture of the three gases, [NH3] = 0.242 M and [ H2] = 1.03 M. What is the concentration of N2 in this system?

Which of the following statements concerning equilibrium constants is true?

Terms relating to certain types of substances are conventionally omitted from equilibrium constant expressions. These substances are

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