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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.
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 (A)
The volume of 1 mole of gas at STP is 22.4 L.
The volume of 1 mole of gas at STP is 22.4 L.
True (A)
The pressure exerted by each gas in a mixture is its partial pressure.
The pressure exerted by each gas in a mixture is its partial pressure.
True (A)
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.
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.
The density of a gas is generally given in g/L.
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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