Final answer:
Increasing temperature increases vapor pressure and does not decrease the equilibrium constant. Increasing atmospheric pressure raises the boiling point, and the partial pressure of vapor depends on temperature. Therefore, statements (a) and (d) are incorrect, while statements (b) and (c) are true.
Step-by-step explanation:
When a liquid is in dynamic equilibrium with its vapor at a given temperature T, several factors can influence the system. Now, let's evaluate the statements presented:
- (a) Increasing temperature will increase vapor pressure, not decrease it. This is because higher temperatures provide more kinetic energy to the liquid molecules, which increases the fraction of molecules that have enough energy to escape into the vapor phase.
- (b) Increasing atmospheric pressure will indeed increase the boiling point. The boiling point is the temperature at which the vapor pressure of a liquid equals the external pressure. So if the atmospheric pressure is increased, the boiling point must also increase to match this pressure.
- (c) The partial pressure of the vapor is dependent on the temperature. As temperature rises, so does the vapor pressure, because a greater fraction of molecules have sufficient energy to escape from the liquid.
- (d) The statement about increasing temperature decreasing the equilibrium constant is incorrect in the context of vapor pressure. The equilibrium constant for a phase change (like vaporization) does not apply here; instead, it is the vapor pressure itself that is temperature-dependent.