The following reaction is at equilibrium in a closed container.
CuSO4.5H2O(s) CuSO4(s) + 5H2O(g)
What actions, if any, will lead to an increase in the pressure of H2O present at equilibrium?
the answer is nothing, but wouldnt decrease in volume will increase pressure
Decrease in volume is an increase in pressure and that will drive the reaction to the left, right? and that will decrease H2O
While it is true that a decrease in volume can generally increase the pressure, in this particular example, there is a solid compound and a gas involved in the equilibrium reaction. Changing the volume of the container will not affect the pressure of the gas phase (H2O) because gases are not affected by changes in volume when in contact with solids or liquids.
In this case, the reaction is at equilibrium in a closed container, which means that it has reached a balance between the reactants and products. Since the pressure of the gas phase is determined by the concentration of the gas, altering the volume alone will not affect the concentration of H2O vapor and, subsequently, its pressure. Therefore, no action will lead to an increase in the pressure of H2O present at equilibrium in this specific situation.