Test: Gaseous State - 5 - Chemistry MCQ

Calculate the volume of O₂ at 1 at m and 273 K required for the complete combustion of 2.64 L of acetylene (C₂H₂) at 1 atm and 273 K. 2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(l)

A certain hydrate has the formula MgSO₄.xH₂O. a quantity of 54.2 g of the compound is heated in an over to drive off the water. If the steam generated exerts a pressure of 24.8 atm in a 2.0 L container at 120°C, calculate x:

A high altitude balloon contains 6.81 g of helium in 1.16 × 10⁴ L at –23°C. Assuming ideal gas behaviour, how many grams of helium would have to be added to increase the pressure to 4.0 × 10^–3 atm:

Starting out on a trip into the mountains, you inflate the tires on your automobile to a recommended pressure of 3.21 × 10⁵ Pa on a day when the temperature is –5°C. You drive to the beach, where the temperature is 28.0°C. Assume that the volume of the tire has increased by 3%. What is the final pressure in the tyres:

Two glass bulbs A and B at same temperature are connected by a very small tube having a stop-cork. Bulb A has a volume of 100 cm³ and contained the gas while bulb B was empty. On opening the stop-cork, the pressure fell down to 20%. The volume of the bulb B is:

Two closed vessel A and B of equal volume of 8.21 L are connected by a narrow tube of negligible volume with open valve. The left hand side container is found to contain 3 mole CO₂ and 2 mole of He at 400 K, what is the partial pressure of He in vessel B at 500 K:

56 g of nitrogen and 96 g of oxygen are mixed isothermally and at a total pressure of 10 at m. The partial pressures of oxygen and nitrogen (in atm) are respectively:

Oxygen gas generated by the decomposition of potassium chlorate is collected over water. The volume of oxygen collected at 24°C and atmospheric pressure of 760 mmHg is 128 mL. Calculate the mass of oxygen gas obtained. The pressure of the water vapour at 24°C is 22.4 mmHg:

Consider three one-litre flasks labeled A, B and C filled with the gases NO, NO₂ and N₂O, respectively, each at 1 atm and 273 K. In which flask do the molecules have the highest average kinetic energy: 

Two flasks A and B have equal volumes. A is maintained at 300 K and B at 600 K, while A contains H₂ gas, B has an equal mass of CO₂ gas. Find the ratio of total K.E. of gases in flask A to that of B:

A mixture of Ne and Ar at 250 K has a total K.E. = 3 kJ in a closed vessel, the total mass of Ne and Ar is 30 g. Find mass % of Ne in gaseous mixture at 250 K

The most probable speed of 8 g of H₂ 200 ms^–1 average kinetic energy (neglect rotational and vibrational energy) of H₂ gas is:

The root mean square speed of 8 g of He is 300 ms^–1. Total kinetic energy of He gas is:

The ratio among most probable velocity, mean velocity and root mean square velocity is given by:

Calculate relative rate of effusion of O₂ to CH₄ through a container containing O₂ and CH₄ in 3:2 mass ratio:

Calculate γ (ratio of C_p and C_v) for triatomic linear gas at high temperature. Assume that the contribution of vibrational degree of freedom is 75%:

If one mole each of a monoatomic and diatomic gases are mixed at low temperature then C_p/C_v ratio for the mixture is:

At low pressures, van der Waal’s equation is written as  The compressibility factor is then equal to:

The temperature at which the second virial coefficient of real gas is zero is called:

The excluded volume of a gas will be larger, if 

A mixture of NH₃(g) and N₂H₄(g) is placed in a sealed container at 300 K. The total pressure is 0.5 atm. The container is heated to 1200 K at which time both substances decompose completely according to the equations

After decomposition is complete, the total pressure at 1200 K is found to be 4.5 atm. Find the mole % of N₂H₄ in the original mixture:

A given volume of ozonised oxygen (containing 60% oxygen by volume) required 220 sec to effuse which an equal volume of oxygen took 200 sec only under the conditions. If density of O₂ is 1.6 g/L then find density of O₃:

The van der Waal’s constant ‘b’ of a gas is 4π × 10^–4 L/mol. How near can the centres of the two molecules approach each other? [Use: N_A = 6 × 10²³]

At a constant pressure, what should be the percentage increase in the temperature in Kelvin for a 10% increase in volume:

For a real gas (mol. mass = 60) if density at critical point is 0.80 g/cm³ and its van der Waal’s constant a (in at m L² mol^–2) is:

A mixture of nitrogen and water vapours is admitted to a flask at 760 torr which contains a sufficient solid drying agent after long time the pressure reached a steady value of 722 torr. If the experiment is done at 27°C and drying agent increases in weight by 0.9 gm, what is the volume of the flask? Neglect any possible vapour of drying agent and volume occupied by drying agent:

Vander Waal’s gas equation can be reduced to virial equation and virial equation (in terms of volume) 

Where A = first virial coefficient, B = second virial coefficient, C = third virial coefficient. The third virial coefficient of Hg(g) is 625 (cm²/mol)². What volume is available for movement of 10 moles He(g) atoms present in 50 L vessel: