In the reactionCO+H20 →CO2 + H2 Δ=-41.84 kJ/mol, if heat is applied at equilibrium stage, it is observed that:
Correct answer: B. The reaction will move in backward direction for compensation
- A. More CO2 and H2 are produced to compensate for temperature change
- B. The reaction will move in backward direction for compensation
- C. No change will take place
- D. The reaction will stop
Explanation
When heat is applied to a system at equilibrium, Le Chatelier's principle states that the system will adjust to counteract the change and restore equilibrium. In this exothermic reaction, heat is considered a product. Therefore, adding heat to the system will shift the equilibrium position to consume the excess heat. Since the forward reaction is exothermic (ΔH = -41.84 kJ/mol), the system will favor the backward reaction (CO2 + H2 → CO + H2O) to consume the added heat. As a result, more CO and H2O will be produced.
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About Thermochemistry and Energetics of Chemical Reactions
Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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