`2CaSO_4(s)hArr2CaO(s)+2SO_2(g)+O_2(g),DeltaH gt 0`
Above equilibrium is established by taking some amount of `CaSO_4(s)` in a closed container at 1600K. Then which of the following may be correct option?
A. Moles of CaSO(s) will increase with increase in temperature.
B. If the volume of the container is doubled at equilibrium then partical pressure of `SO_2(g)` will change at new equilibrium
C. If the volume of the container is halved 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.
