A container holds a volume of 1.0 cm3 of liquid nitrogen at its boiling point of −196 ∘C-196\text{ }^\circ\text{C}−196 ∘C. Upon boiling, the nitrogen vaporizes to form approximately 700 cm3 of nitrogen gas at room temperature and pressure.
What is the primary reason for this large increase in volume?
Nitrogen gas molecules are significantly larger than liquid nitrogen molecules.
The average distance between the molecules is much greater in the gaseous state than in the liquid state.
There are many more molecules of nitrogen in the gas than there were originally in the liquid.
The nitrogen molecules do not move at all while in the liquid phase.
321 exam-style questions on CIE IGCSE Physics 2.1 Kinetic particle model of matter, covering 2.1.1 States of matter and changes of state, 2.1.2a Particle structure and motion in solids, liquids and gases, 2.1.2b Gas pressure and particle collisions, 2.1.2c Brownian motion, 2.1.3a The absolute scale of temperature, and 2.1.3b Pressure, volume and temperature of a gas. Each one has a worked solution and a mark scheme showing where the marks go.