For `H_(2)` gas, `a=0.024L^(2)*atm*mol^(-2),`
`b=0.026L*mol^(-1) and ` for `CH_(4)` gas:
`a=2.28L^(2)*atm*mol^(-2)`, `b=0.042L*mol^(-1)`.
(i) At ordinary temperature and pressure, which one of the two gases will behave more like an ideal gas?
(ii) Which one of the two gases has a larger molecular size?

Explanation

(i) At ordinary temperature and pressure, a ral gas behaves more like an ideal gas if the values of 'a' and 'b' are very small. The values of 'a' and 'b' for `H_(2)` gas are smaller than those for `CH_(4)` gas. Obviously, at ordinary temperature and pressure, `H_(2)` gas will behave more like an ideal gas.
(ii) The value of 'b' for a real gas reflects the sizes of molecules of the gas. a goas whose molecules are large in size has a high value of 'b' as the value of 'b' for `CH_(4)` gas is greater than that of `H_(2)` gas, the size of `CH_(4)` molecule will be larger than that of `H_(2)` molecule.