Chapter 1

An evacuated bulb of unknown volume is filled with a sample of \(\mathrm{H}_{2}\) gas at a temperature \(T\). The pressure of the gas in the bulb is \(756 \mathrm{~mm} \mathrm{Hg}\). A portion of the \(\mathrm{H}_{2}\) gas is transferred to a different flask and found to occupy a volume of \(40.0 \mathrm{~mL}\) at \(1.00\) atm and the same temperature \(T\). The pressure of the \(\mathrm{H}_{2}\) gas remaining in the original bulb drops to 625 \(\mathrm{mm} \mathrm{Hg}\) at the same temperature \(T\). Assuming \(\mathrm{H}_{2}\) is an ideal gas, what is the volume of the bulb?

An open flask contains air at \(27^{\circ} \mathrm{C}\). Calculate the temperature at which it should be heated so that, (a) \(\frac{1}{3} \mathrm{rd}\) of air measured at \(27^{\circ} \mathrm{C}\) escapes out. (b) \(\frac{1}{3} \mathrm{rd}\) of air measured at final temperature escapes out.

A bulb of three litre capacity filled with air is heated from \(27^{\circ} \mathrm{C}\) to \(t^{\circ} \mathrm{C}\). The air thus, expelled measured \(1.45\) litre at \(17^{\circ} \mathrm{C}\). Considering the pressure to be 1 atm throughout the experiment and ignoring the expansion of bulb, calculate \(t\).

One litre of a gas at 300 atm and \(473 \mathrm{~K}\) is compressed to a pressure of 600 atm and \(273 \mathrm{~K}\). The compressibility factors found to be \(1.072\) and \(1.375\) respectively at the initial and finally conditions. Calculate the final volume.

Calculate the relative rates of diffusion for \({ }^{235} \mathrm{UF}_{6}\) and \({ }^{238} \mathrm{UF}_{6}\).

Equal volumes of two gases \(A\) and \(B\) diffuse through a porous pot in 20 and 10 seconds respectively. If the molar mass of \(A\) be 80, find the molar mass of \(B\)