Consider the following reaction: 2CO(g) + O2(g) ---> 2CO2(g)?
Imagine that this reaction occurs in a container that has a piston that moves to allow a constant pressure to be maintained when the reaction occurs at constant temperature. (a) What happens to the volume of the container as a result of the reaction? Explain. (b) If the piston is not allowed to move, what happens to the pressure as a result of the reaction?
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Note that, in that reaction, 3 moles of gaseous reactants become 2 moles of gaseous product, so if temperature is maintained constant and there is a sliding piston, the volume will decrease. This is assuming the non-reactant side of the pistion is exposed to the air or some other non-changing pressure. If the piston is prevented from moving, and T is constant, you will have 2 moles of gas occupying the same volume that originally had 3 moles, so the pressure will decrease.