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Question

2CaSO4(s)2CaO(s)+2SO2(g)+O2(g),ΔH>0
Above equilibrium is established by taking a sufficient amount of CaSO4(s) in a closed container at 1600 K. Then which of the following may be the correct option(s)?
(Assume that solid CaSO4 is present in the container in each case)

A
Moles of CaO(s) will increase with the increase in temperature
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B
If the volume of the container is doubled at equilibrium then partial pressure of SO2(g) will change at new equilibrium
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C
If the volume of the container is halved partial pressure of O2(g) at new equilibrium will remain same
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D
If two moles of He gas is added at constant pressure then the moles of CaO(s) will increase.
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Solution

The correct options are
A Moles of CaO(s) will increase with the increase in temperature
C If the volume of the container is halved partial pressure of O2(g) at new equilibrium will remain same
For endothermic reaction (ΔH>0) if temperature increases equilibrium shift towards the right. Therefore option A is correct.
For any change in the volume of the container is not going to change the equilibrium pressure at a given temperature if the CaSO4 is available. Therefore partial pressure of SO2 will not change. B incorrect.
Same reason as for B. Option C is correct.
If any external gas is added to the equilibrium at a constant pressure it will shift towards left. Thus option D is wrong.

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