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. 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
Step 1
A. The concentration of COCl\(_2\) would increase.
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Answer
Heating an equilibrium system generally favors the endothermic direction if the reaction's enthalpy is known. COCl(_2) will not necessarily increase without understanding the balanced reaction.
Step 2
B. The total gas pressure in the flask would decrease.
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Answer
According to the ideal gas law, increasing the temperature at constant volume will actually increase the pressure, not decrease it.
Step 3
C. The equilibrium constant for the reaction would increase.
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Answer
The equilibrium constant depends on temperature. For endothermic reactions, increasing temperature will increase the equilibrium constant of the system.
Step 4
D. The total number of gas molecules in the flask would increase.
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Answer
The total number of gas molecules does not change simply due to increased temperature at constant volume; the stoichiometric relationships based on the reaction must be considered.
