If the equilibrium system were suddenly heated at constant volume at the five-minute mark, which one of the following changes would result? A. The concentration of COCl2 would increase. B. The total gas pressure in the flask would decrease. C. The equilibrium constant for the reaction would increase. D. The total number of gas molecules in the flask would increase.

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If the equilibrium system were suddenly heated at constant volume at the five-minute mark, which one of the following changes would result? A - VCE - SSCE Chemistry - Question 16 - 2016 - Paper 1

Question 16

If-the-equilibrium-system-were-suddenly-heated-at-constant-volume-at-the-five-minute-mark,-which-one-of-the-following-changes-would-result?--A-VCE-SSCE Chemistry-Question 16-2016-Paper 1.png

If the equilibrium system were suddenly heated at constant volume at the five-minute mark, which one of the following changes would result? A. The concentration of ... show full transcript

Worked Solution & Example Answer:If the equilibrium system were suddenly heated at constant volume at the five-minute mark, which one of the following changes would result? A - VCE - SSCE Chemistry - Question 16 - 2016 - Paper 1

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C. The equilibrium constant for the reaction would increase.

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When a system at equilibrium is heated, according to Le Chatelier's principle, the equilibrium will shift in the direction that absorbs heat to counteract the temperature increase. For an endothermic reaction, this means that the equilibrium constant will increase because the forward reaction is favored, resulting in more products. Therefore, option C is correct.

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