What is difference between vapour pressure and partial pressure?

Answer: Partial pressure is the pressure exerted by an object, whereas vapour pressure is the pressure exerted by a gas. While the vapour pressure refers to the pressure that the vapour exerts when it is in thermodynamic equilibrium with its condensed state of liquid, each individual gas in a mixture acts as if it were acting alone in that system. An ideal gas mixture’s total pressure is equal to the sum of its constituent gases’ individual partial pressures. The thermodynamic activity of a gas’s molecules is gauged by its partial pressure.

The gas’s vapour pressure: vapour pressure is the force applied by this gas phase when it is in equilibrium with its solid or liquid equivalent. If a bottle of water is heated, for instance, both the pressure and the amount of water vapour will rise.

The gas’s partial pressure is: each constituent gas in a mixture of gases has a partial pressure, which is the notional pressure of that constituent gas at the same temperature if it occupied the entire volume of the original mixture on its own. The thermodynamic activity of a gas’s molecules is gauged by its partial pressure.