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. low temperature and high pressure.
Explanation
A2(g)+ 4B2(g) ⇌ 2AB4(g) ∆H = -Ve 5mole 2mole 5 volume 2 volume According to Le-Chatelier principle, for exothermic reactionYield ∝ 1 /TemperatureAnd increase in pressure move reaction in direction in which volume in less. Because reactant have more volume than product so increase in pressure favours forward reaction.
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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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