State one similarity and one difference in how the atoms in a carbon monoxide molecule are bonded together compared with the atoms in a nitrogen molecule.
Use the electronegativity values and the relevant details from the Data Booklet to fill in the table comparing $\mathrm{N_2}$ and $\mathrm{CO}$ for electrons per molecule and the type(s) of intermolecular (van der Waals') force.
$\mathrm{N_2(g)}$ is less reactive than $\mathrm{CO(g)}$ even though $\mathrm{N_2(g)}$ has a lower bond energy than $\mathrm{CO(g)}$. Suggest why $\mathrm{CO(g)}$ is more reactive than $\mathrm{N_2(g)}$.
State the two conditions needed for these two gases to approach ideal gas behaviour.
Explain why $\mathrm{N_2(g)}$ behaves more like an ideal gas than $\mathrm{CO(g)}$ does at $20.0\,^{\circ}\mathrm{C}$ and $101\,\text{kPa}$.
Calculate the amount, in $\text{mol}$, of pure nitrogen gas that occupies $100\,\text{cm}^3$ at $101\,\text{kPa}$ and $20.0\,^{\circ}\mathrm{C}$. Use relevant information from the Data Booklet. Show your working. Assume nitrogen behaves as an ideal gas.