On the axes, draw a curve to represent the Boltzmann distribution of energy for particles in a sample of gaseous krypton atoms at a fixed temperature. Mark the curve $T1$ and label the axes.
In (a)(i), draw a second curve on the diagram to show the energy distribution of the krypton atoms at a higher temperature. Label the second curve $T2$.
State two assumptions made by the kinetic theory when it is applied to an ideal gas.
A mass of 2.00 g of krypton gas, $\text{Kr}(g)$, is put into a sealed $5.00\ \text{dm}^3$ container at $120\,^{\circ}\text{C}$. Calculate the pressure, in Pa, of $\text{Kr}(g)$ in the container. Assume $\text{Kr}(g)$ behaves as an ideal gas. Show your working.
State and explain the conditions under which krypton behaves most like an ideal gas.
Krypton reacts with fluorine under ultraviolet light to form krypton difluoride, $\text{KrF}_2(g)$. The reaction is $\text{Kr}(g) + \text{F}_2(g) \rightarrow \text{KrF}_2(g)$. The activation energy is $E_a = +385\ \text{kJ mol}^{-1}$ and the enthalpy change of formation of $\text{KrF}_2$ is $\Delta H_f = +60.2\ \text{kJ mol}^{-1}$. Use these details to complete the reaction profile diagram for the formation of $\text{KrF}_2$. Put labels for $E_a$ and $\Delta H_f$ on the diagram. Assume the reaction happens in one step.
Explain, in terms of activation energy, $E_a$, and the collision of particles, how an increase in temperature affects the rate of a chemical reaction.