Question

In which of the following conditions, the distance between the molecules of hydrogen gas would increase?

(i) Increasing pressure on hydrogen contained in a closed container.
(ii) Some hydrogen gas leaking out of the container.
(iii) Increasing the volume of the container of hydrogen gas.
(iv) Adding more hydrogen gas to the container without increasing the volume of the container.

• A. (i) and (iii)
• B. (i) and (iv)
• C. (ii) and (iii)
• D. (ii) and (iv)

Answer 1

The correct option is C (ii) and (iii)

As per ideal gas law, $PV=nRT$, $i.e.$ pressure is directly proportional to temperature and indirectly proportional to the volume of a closed container, and intermolecular forcesare forces of attraction or repulsion which act between neighbouring particles (atoms, molecules or ions).

(i) Increasing pressure on hydrogen contained in a closed container would decrease the distance between the molecules of hydrogen gas, Thus this option is not possible.

(ii) Some hydrogen gas leaking out of the container would accommodate more space so the distance between the molecules of hydrogen gas would increase, thus it is the correct answer.

(iii) Increasing the volume of the container of hydrogen gas would also accommodate more space so the distance between the molecules of hydrogen gas would increase, thus it is also the correct answer.

(iv) Adding more hydrogen gas to the container without increasing the volume of the container would take the space of existing molecules so the distance between the molecules of hydrogen gas would decrease. Thus it is also incorrect answer.

Hence, the correct option is $\text{C}$