Question

Consider the reaction between NO and NO to produce the dimer N2O2. It the reaction is at equilbirium in a closed container, which way will the reaction proceed if the volume of the container is halved? 2NO(g)↔N₂O₂(g)

A No change

B Reaction will make more N2O2

C Reaction will make more NO

The ΔH for vaporization of water at 25oC is 44.0. What change will occur to the equilibrium between vapor and liquid in a closed container when the temperature is increased. H2O(l)↔H2O(g)

A No change

B More Water will evaporate

C More water will condense

Answer 1

1. Sice reactant moles are double than product moles. Decreasing volume means from boyles law (PV=constant) we are increasing pressure, hence more product formed.

Answer: B Reaction will make more N2O2

2. Even though we are performing in a closed vessel increasing temperature makes water molecules to be more kinetic energy. Due to thermal motion, the molecules inside the control volume try to expand into gas phase, but since the gas phase pressure at that temperature is lower than the pressure by liquid, it can't expand. But as soon as the pressure exerted by the liquid becomes equal to the gas pressure, the molecules inside can easily transform into gas phase.

Answer: B More Water will evaporate

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