ANS:C - partial pressure

Partial pressure is a concept used to describe the pressure exerted by a single component of a mixture of gases, assuming that the other components are held constant. In other words, it represents the pressure that a gas component would exert if it occupied the entire volume alone, under the same conditions as the mixture. Here's a more detailed explanation of partial pressure:

1. Mixture of Gases: When a gas mixture contains two or more different gases, each gas contributes to the total pressure exerted by the mixture. The total pressure of the gas mixture is the sum of the partial pressures of its individual components.
2. Dalton's Law of Partial Pressures: Dalton's law states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases. Mathematically, it can be expressed as: 𝑃total=𝑃1+𝑃2+𝑃3+…Ptotal​=P1​+P2​+P3​+… Where:
   • 𝑃totalPtotal​ is the total pressure of the gas mixture.
   • 𝑃1,𝑃2,𝑃3,…P1​,P2​,P3​,… are the partial pressures of the individual gas components.
3. Units: Partial pressure is typically expressed in the same units as total pressure, such as atmospheres (atm), pascals (Pa), millimeters of mercury (mmHg), or torr.
4. Determining Partial Pressure: The partial pressure of a gas component can be determined by multiplying the mole fraction of that component by the total pressure of the mixture. Mathematically, it can be expressed as: 𝑃component=𝑥component×𝑃totalPcomponent​=xcomponent​×Ptotal​ Where:
   • 𝑃componentPcomponent​ is the partial pressure of the gas component.
   • 𝑥componentxcomponent​ is the mole fraction of the gas component in the mixture.
   • 𝑃totalPtotal​ is the total pressure of the gas mixture.