At moderate pressure, the Vander waal's equation becomes:-

The compressibility factor for a real gas at high pressure is:-

1.6 g O₂ gas and 0.1 g H₂ gas are placed in a 1.12 L flask at 0 ^oC. The total pressure of the gas mixture will be-

1. 2 atm

Rate of diffusion of LPG (a mixture of n-butane and propane) is 1.25 times of SO₃. Hence, mass fraction of n-butane in LPG is

An open flask containing air is heated from 300 K to 500 K. The percentage of air that will escape into the atmosphere if pressure is kept constant is-

V versus T curves at constant pressure P₁ and P₂ for an ideal gas are as shown in the figure. The correct statement is-

A spherical balloon of 21 cm dimeter is to be filled up with H₂ at NTP from a cylinder containing the gas at 20 atm at 27^o The cylinder can hold 2.82 litre of water at NTP. Calculate the number of balloons that can be filled up.

A 20 g chunk of dry ice is placed in an empty 0.75 litre bottle and tightly closed.  The final pressure in the bottle after all CO₂ has been evaporated and temperature reaches to 25^oC is-

A mixture of CO and CO₂ is found to have a density  1.5 g/litre at 30^oC and 730 mm. The composition of the mixture is-

A collapsed polythene bag of 30 litre capacity is partially blown up by the addition of 10 litre of N₂ at 0.965 atm at 298 K. Subsequently,  enough O₂  is pumped into bag so that at 298 K and external pressure of 0.990 atm, the bag contains full 30 litre. The final pressure of O₂ in the following experiment is-

A 40 mL of a mixture of H₂ and O₂ was placed in a gas burette at 18 ^oC and  1 atm pressure. A spark was supplied so that the formation of water was complete . The remaining pure gas had a volume of 10 mL at 18 ^oC  and 1 atm pressure. If the remaining gas was H₂ , what was the initial mole percentage of H₂ in the mixture?

60 mL of a mixture of equal volume of Cl₂ and an oxide of chlorine was heated and then cooled back to the original temperature. The resulting gas mixture was found to have volume of 75 ml. On treatment with caustic soda solution, the volume contracted to 15 ml. Assume that all the measurements are made at same T and P. Deduce the simplest formula for oxide of Cl₂. The oxide of Cl₂ on heating decomposes quantitatively to O₂ and Cl₂.

For the reaction, N₂ O₅  (g)→2NO₂ (g) + 0.5 O₂ (g),

Calculate the mole fraction of N₂ O₅ (g) decomposed at a constant volume and temperature if the initial pressure is 600 mm Hg and the pressure at any time is 960 mm Hg.  Assume ideal gas behaviour.

An underwater bubble with radius of  5 cm at the bottom of tank , where the temperature is 5^oC and pressure is 3 atm rises to the surface, where temperature is 25 ^oC and pressure is 1 atm. What will be the radius of bubble when it reaches to the surface?

If density of vapours of a substance of molar mass 18 g/mole at 1 atm pressure and 500 K is

0.36 kg m^–3 , then the value of Z for the vapours is-

(R = 0.082 L atm mole K^–1)

Equal amount (mass) of methane and ethane have their total translational kinetic energy in the ratio

3: 1 then their temperatures are in the ratio.

The graph that represents an isobar $\left(\frac{\mathrm{nR}}{\mathrm{p}}\mathrm{\hspace{0.17em}}>\mathrm{\hspace{0.17em}1}\right)$ is-

For a certain gas which deviates a little from ideal behaviour, the values of density, p

were measured at different values of pressure, P. The plot of P/p on the Y–axis versus P on the X–axis was nonlinear and had an intercept on the Y–axis, which was equal to

Where M = molar mass.

A sample of water gas has a composition by volume of 50% H₂, 45% CO and 5% CO₂. Calculate the volume in litre at S.T.P. of water gas which on treatment with excess of stream will produce 5 litre H₂. The equation for the reaction is : CO + H₂O $\stackrel{}{\to }$ CO₂+ H₂

Flask A of volume 10 litre containing 20 gram of H₂ and flask B of volume 10 litre containing 88 gram CO₂ are connected by a connector having negligible volume. When the valve of the connector is opened, the composition of H₂ gas in flask B after opening the valve is-

A mixture of two gases A and B in the mole ratio 2 : 3 is kept in a 2 litre vessel. A second 3 litre vessel has the same two gases in the mole ratio 3 : 5. Both gas mixtures have the same temperature and same total pressure. They are allowed to intermix ,the final temperature and total pressure are the same as the initial values, the final volume being 5 litres. Given that the molar masses are M_A and M_B, what is the mean molar mass of the final mixture?

A 2 m long tube closed at one end is lowered vertically into' water until the closed end is flush with the water surface. See figure below. Calculate the water level height in the tube. (Barometric pressure –1 atm =10 m of hydrostatic water head, Temperature = 25°C, Density of, water = 1.00 g/ml. Neglect water vapour pressure).

At a certain temperature for which RT = 25 lit. atm. mol^–1, the density of a gas, in gm lit^–1, is d = 2.00P + 0.020 P², where P is the pressure in atmosphere. The molecular weight of the gas in gm mol^–1 is-

A mixture of carbon monoxide and carbon dioxide is found to have a density of 1.7 g/L at S.T.P. The mole fraction of carbon monoxide is-

The van der Waal's constant 'b' for N₂ and H₂ has the values 0.039 lit moil^–1 and 0.0266 lit mo1^–1. The density of solid N₂ is 1 g cm^–3. Assuming the molecules in the solids to be close packed with the same percentage void, the density of solid H₂ would be (in g cm^–3)

A certain gas effuses out of two different vessels A and B. A has a circular orifice while B has a square orifice of length equal to the radius of the orifice of vessel A. The ratio of rate of diffusion of the gas from vessel A to that from vessel B is

A sample of a given mass of a gas at a constant temperature occupies 95cm³ under a pressure of $9.962\times {10}^4{\mathrm{Nm}}^{-2}$. At the same temperature, the volume at a pressure of $10.13\times {10}^4{\mathrm{Nm}}^{-2}$ is [Bihar CEE 1992]

A gas occupied a volume of 250 ml at 700 mm Hg pressure and 25°C. An additional pressure is required to reduce the gas volume to its 4/5^th value at the same temperature is-

At constant temperature, if pressure increases by 1%, the percentage decrease of volume is-

When the temperature of 23 ml of dry CO₂ gas is increased from 10° to 30°C at a constant pressure of 760 mm, the volume of gas becomes-