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States of Matter
Dalton's Law of Partial Pressures
5 questions from 5 papers, each with its answer.
- questions
- 5
- papers
- 5
- years asked, 2017–2026
- 4 of 10
- of States of Matter
- 14.29%
Appears in
Concepts tested
- Dalton's law of partial pressures
- mathematical forms of Dalton's law
- Partial pressure
- partial pressure from mole fraction
- total pressure of a gas mixture
All Questions
2022 1 question
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Which one is not correct mathematical equation for Dalton's Law of partial pressure? Here $p$ = total pressure of gaseous mixtureDalton's law: partial pressure of a gas = mole fraction × total pressure of the mixture. $p_1 = x_1p$, $p_2 = x_2p$, $p_3 = x_3p$ and $p = p_1 + p_2 + p_3$ (also $p = n_1\frac{RT}{V} + n_2\frac{RT}{V} + n_3\frac{RT}{V}$) $p_i = x_ip_i^\circ$ (with $p_i^\circ$ = pressure of the pure component) is the form of Raoult's law, not Dalton's law – so it is not correct.
2021 1 question
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Choose the correct option for the total pressure (in atm.) in a mixture of 4 g $O_2$ and 2 g $H_2$ confined in a total volume of one litre at $0^\circ C$ is: [Given $R=0.082\ L\ atm\ mol^{-1}K^{-1}$, $T=273\ K$]$n_{O_2} = \frac{4}{32} = \frac{1}{8}$ mol ; $n_{H_2} = \frac{2}{2} = 1$ mol ; $n_{total} = \frac{9}{8}$ mol $PV = nRT \Rightarrow P \times 1 = \frac{9}{8} \times 0.082 \times 273$ $P_{total} = 25.18$ atm
2020 1 question
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A mixture of $N_2$ and Ar gases in a cylinder contains 7 g of $N_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of $N_2$ is: [Use atomic masses (in $g\,mol^{-1}$): N = 14, Ar = 40]$n_{N_2} = \frac{7}{28} = 0.25$ mol ; $n_{Ar} = \frac{8}{40} = 0.20$ mol By Dalton's law: $p_{N_2} = \chi_{N_2}P_{total} = \frac{0.25}{0.45} \times 27$ $= \frac{5}{9} \times 27 = 15$ bar
2019 Odisha 1 question
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In water saturated air the mole fraction of water vapour is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is:Mole fraction of dry air $=1-0.02=0.98$. Partial pressure $=1.2\times0.98=1.176$ atm.
2011 AIPMT-PRE 1 question
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A gaseous mixture was prepared by taking equal moles of CO and $N_2$. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen ($N_2$) in the mixture isDalton's law: partial pressure of a gas = mole fraction of the gas × total pressure.
Let the moles of CO = moles of $N_2$ = n.
Mole fraction of $N_2$ = $\frac{n}{n + n} = \frac{1}{2}$
$p_{N_2} = \frac{1}{2}\times1$ atm
$p_{N_2} = 0.5$ atm