During an experiment, a sample of a pure gas is placed in a gas syringe at a temperature of $300\,\text{K}$ and a pressure of $16\,\text{kPa}$. The gas is then compressed so that the volume it occupies is reduced by half. Once compression has taken place, the gas in the syringe has a temperature of $375\,\text{K}$ and a pressure of $40\,\text{kPa}$. Which statement is correct?
- AIntermolecular forces between the gas molecules are significant.
- BIt is possible to calculate the number of moles of gas present using these data alone.
- CThe gas is behaving ideally.
- DThe pressures used are too high for ideal gas behaviour.