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24 April, 05:57

Consider this system at equilibrium.

A (aq) B (aq) deltaH=-750kJ/mol

What can be said about Q and K immediately after an increase in temperature?

A) Q>K because Q increased

B) Q>K because K decreased

C) Q D) Q E) Q=K because neither charged

How will the system respond to a temperature increase?

A) shift left

B) shift right

C) no change

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Answers (1)
  1. 24 April, 05:59
    0
    a) Q>K because K decreased

    b) shift left

    Explanation:

    According to Van't Hoff equation

    d (ln K) / dT = ΔH/RT²

    since ΔH< 0 (exothermic reaction), then d (ln K) / dT < 0 → K decreases with an increase in temperature

    thus

    a) Since Q represents the product of concentrations, and assuming an increase in temperature do not affect significantly the concentration of products in a liquid state, then Q remains approximately constant, but K decreases → Q>K because K decreased

    (thus ΔG is positive and ΔG is negative for the reverse reaction → products will produce reactants until the new equilibrium is reached)

    b) Since K decreased, the system will shift towards the reactants and thus it will shift to the left
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