A gaseous mixture contains 56 g of N2, 44 g of CO2 and 16 g of CH4. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH4 is-
1. 180 mm
2. 360 mm
3. 540 mm
4. 720 mm
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The partial pressure of oxygen in a flask containing 16 g and 32 g is-
1. 1/16 of total pressure
2. 1/2 of total pressure
3. 2/3 of total pressure
4. None of the above
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In a flask of volume V litres, 0.2 mol of oxygen, 0.4 mol of nitrogen, 0.1 mol of ammonia and 0.3 mol of helium are enclosed at . If the total pressure exerted by these non-reacting gases is one atmosphere, the partial pressure exerted by nitrogen is-
1. 1 atm
2. 0.1 atm
3. 0.2 atm
4. 0.4 atm
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Equal weights of ethane and hydrogen gas are mixed in an empty container at . The fraction of total pressure exerted by hydrogen is-
1. 1: 2
2. 1: 1
3. 1: 16
4. 15: 16
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The partial pressure of H2 in a flask containing 2 g of H2, 14 g of N2, and 16 g of O2 is-
1. 1/2 of the total pressure
2. 1/3 of the total pressure
3. 1/4 of the total pressure
4. 1/16 of the total pressure
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Which among the following mixtures of gases at room temperature does not obey Dalton's law of partial pressure-
1. He and O2
2. NH3 and HCl
3. H2 and He
4. N2 and He
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Equal weights of methane and oxygen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is-
1. 1/3
2. 1/2
3. 2/3
4.
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In water-saturated air, the mole fraction of water vapor is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is-
1. 1.17 atm
2. 1.76 atm
3. 1.27 atm
4. 0.98 atm
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At STP, a container has 1 mole of He, 2 moles Ne, 3 moles of , and 4 moles . Without changing total pressure if 2 moles of is removed, the partial pressure of will be decreased by-
1. 26 %
2. 40 %
3. 58.33 %
4. 66.66 %
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The pressure of a 1 : 4 mixture of dihydrogen and dioxygen enclosed in a vessel is one atmosphere. The partial pressure of dioxygen is-
1.
2.
3.
4.
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