What effect does increasing temperature have on boiling point?

Increasing temperature generally leads to an increase in boiling point due to the principles of vapor pressure and atmospheric pressure. As the temperature of a liquid rises, its molecules gain kinetic energy, which allows more of them to escape from the surface and enter the vapor phase. However, the boiling point is defined as the temperature at which the vapor pressure of the liquid equals the surrounding atmospheric pressure.

When the temperature increases, if the atmospheric pressure remains constant, the vapor pressure of the liquid will also increase. If the liquid reaches a point where its vapor pressure matches the atmospheric pressure, it begins to boil. Therefore, if you consider the effects of increased temperature on a given substance under normal atmospheric conditions, you can expect that the substance will require a higher temperature to boil.

It is important to note that under varying atmospheric pressures (for instance, at higher elevations where the pressure is lower), the relationship might change and boiling points can decrease, but this is not typically what is meant when discussing the effect of increased temperature. So, in a controlled setting such as a laboratory, where pressure is generally assumed to be constant, increasing temperature indeed leads to an increase in boiling point for a liquid.