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Ideal Gas Equation

States of Matter
Chemistry
Class 11

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Ideal Gas Equation

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Dalton's Law of Partial Pressures

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For minute each, at C, from two identical holes nitrogen and an unknown gas are leaked into a common vessel of litre capacity. The resulting pressure is atm and the mixture contains mole of nitrogen. What is the molar mass of unknown gas? (Use L-atm/mol-K).

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Which of the following pair of gases will have same rate of diffusion under similar conditions?

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of a gas is changed from its initial state to final state reversinly. If this change can be represented by a straight line in curve, calculate maximum temperature, the gas attained.

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Which one of these graphs for an ideal gas, the arrow indication is incorrectly marked? 

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A rigid tank contains of nitrogen at . Sufficient quantity of oxygen is supplied to increase the pressure to , while the temperature remains constant. Amount of oxygen supplied to the tank is :

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Vapour pressure of chloroform and dichloromethane at are 200 mm Hg and 415 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of and 40 g of at the same temperature will be:

[Molecular mass of and molecular mass of ]

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Calculate pressure of gas whose molar mass is having density at 273 K.

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The molar volume of liquid benzene () increases by a factor of as it vaporizes at  C and that of liquid toluene ()increases by a factor of at  C. A solution of benzene and toluene has a vapour pressure of torr. Find the mole fraction of benzene in the vapour above the solution:

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An ideal gas occupying a volume of 2 d and a pressure of 5 bar undergoes isothermal and irreversible expansion against external pressure of 1 bar. The final volume of the system and the work involved in the process is

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An evacuated glass vessel weights 50.0 g when empty.  148.0 gm when filled with a liquid of density 0.98 g/mL and 50.5 g when filled with an ideal gas at 760 mm Hg at 300 K. Determine the molecular weight of the gas.

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