States of Matte...

Direction (Q. Nos. 1-12) This section contains 12 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.

Q. 
The vapour pressure of liquid water is 23.8 torr at 25°C. By what factor does the molar volume of water increases as it vaporises to form an ideal gas under these conditions? The density of liquid water is 0.997 g cm^-3 at 298 K ?

A gas at a pressure of 5.0 bar is heated from 0°C to 546°C and is simultaneously compressed to one-third of its original volume. Hence, final pressure is

A 8.3 L cylinder contains 128 . 0 g O₂ gas at 27°C. What mass of O₂ gas must be released to reduce the pressure to 6.0 bar ?

 N₂ gas under the given state I is to be changed to state II. Thus, N₂ escaped from I is 

1 g H₂ gas and x g O₂ gas exert a total pressure of 5 atm. At a given temperature partial pressure of O₂ gas is 4 atm. This O₂ in the mixture is 

The average molar mass of the vapour above solid NH₄CI is nearly 26.75 g mol^-1.

Thus, vapour consists of (mole fraction)

Pressure of 1 g of an ideal gas A at 300 K is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at the same temperature, pressure becomes 3 bar. Thus,

Total pressure of a mixture of H₂ and O₂ is 1.00 bar. The mixture is allowed to react to form water, which is completely removed to leave only pure l-l₂ at a pressure of 0.35 bar. Assuming ideal gas behaviour and that all pressure measurements were made under the same temperature and volume conditions, the composition of the original mixture is

The composition of air inhaled by a human is 21 % by volume O₂ and 0.03% CO₂ and that of exhaled air is 16% O₂ and 4.03% CO₂. Assuming a typical volume of 6200 L day ^-1, moles of O₂ used and CO₂ generated by the body at 37°C and 1.00 bar are (assume ideal behaviour)

The following arrangement of flasks is set up. Assuming no temperature change, determine the final pressure inside the system after all stopcocks are opened. The connecting tube has zero volume.
 

1.00 mole sample of O₂ and 3.00 moles sample of H₂ are mixed isothermally in a 125.3 L container at 125°C. Gaseous mixture undergoes reaction to form water vapours. Assume ideal gas behaviour total pressure before and after H₂O (g) is formed is are respectivel

When NO₂ is cooled to room temperature, some of it reacts to form a dimer N₂O₄ through the reaction,

In a reaction, 15.2 g of NO₂ is placed in a 10.0 L flask at high temperature and the flask is cooled to 25°C. The total pressure is measured to be 0.500 atm. Thus, partial pressure of NO₂ is found to be