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Questions and Answers
According to Dalton’s law of partial pressures, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.
True
The volume of 1 mole of gas at STP is 22.4 L.
True
The pressure exerted by each gas in a mixture is its partial pressure.
True
The pressure exerted by the hydrogen gas in the cylinder can be determined using the equation $P_{ ext{total}} = P_{ ext{H}2O} + P{ ext{H}2}$, where $P{ ext{H}2O}$ is the vapor pressure of water and $P{ ext{H}_2}$ is the pressure of the hydrogen gas.
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The density of a gas is generally given in g/L.
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Study Notes
Gas Mixtures and Partial Pressures
- Total pressure of a gas mixture equals the sum of partial pressures of its component gases (Dalton's law).
- Partial pressure is the pressure exerted by each gas in a mixture.
Gas Properties
- Volume of 1 mole of gas at Standard Temperature and Pressure (STP) is 22.4 L.
- Density of a gas is typically expressed in grams per liter (g/L).
Pressure Equations
- Pressure of a gas mixture can be determined using the equation: $P_{total} = P_{H_2O} + P_{H_2}$
- $P_{H_2O}$ represents vapor pressure of water, while $P_{H_2}$ is the pressure of hydrogen gas.
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Description
Test your knowledge on the density of gases at STP and Dalton's law of partial pressures in physical chemistry and biochemistry. This quiz covers concepts such as mass to volume ratio, molar mass, and properties of specific gases at STP.
