`2CaSO_4 (s) hArr 2CaO(s)+2SO_(2)(g)+O_2(g), DeltaHgt0`
Above equilibrium is establised by taking some amount of `CaSO_4(s)` in a closed container at 1600 K. Then which of the following may be correct options ?

Options

A. Moles of `CaO(s)` will increase with the increase in temperature
B. If the voulme of the container is doubled at equilibrium then partial pressure of `SO_(2)(g)` will change at new equilibrium
C. If the volume of the container is halved partial pressure of `O_(2)(g)` at new equilibrium will remain same
D. If two moles of the He gas is added at constant pressure then the moles of `CaO(s)` will increase.

Answer

A, C, D

Explanation

(A) As reaction is endothermic therefore it will go in the forward direction hence moles of `CaO` will increase.
(B) With the increase or decrease of volume partial pressure of the gases will remain same.
(C) Due to the addition of inert gas at constant pressure reaction will proceed in the direction in which more number of gaseous moles are formed.