In the reaction A₂(g) + 4B₂(g) ⇌ 2AB₄(g) such that ∆H is negative, the formation of AB₄(g) will be favored 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
The reaction is exothermic (ΔH is negative), so low temperature favors the forward reaction. The reaction goes from 5 moles of gas to 2 moles of gas, so high pressure favors the side with fewer moles, which is also the 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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