In the reaction A2(g)+ 4B2(g) ⇌ 2AB4(g) such that ∆H is negative, the formation of AB4(g) will be favoured at:
Correct answer: A. Low temperature and high-pressure.
- A. Low temperature and high-pressure.
- B. Low temperature and low pressure.
- C. High temperature and high pressure.
- D. High temperature and low pressure.
Explanation
Low temperature: Since the reaction is exothermic (ΔH<0), lowering temperature favors the forward reaction (formation of AB₄) to produce heat and restore balance.High pressure: The reaction goes from 5 moles of gas (1 + 4) to 2 moles of gas (products). Increasing pressure favors the side with fewer gas moles to reduce pressure, so it favors formation of AB₄.Overall: This condition favors the formation of AB₄.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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