Use the figures in the table to work out the order for each reactant. Show how you arrive at your answer.
Calculate the initial rate in experiment $4$. Give your answer to two significant figures.
Write the rate equation that applies to this reaction.
Use the results of experiment $1$ to calculate the rate constant, $k$, for this reaction. Include the units of $k$.
On the axes below, draw two Boltzmann distribution curves for two different temperatures, $T_1$ and $T_2$ ($T_2 > T_1$), and label both the curves and the axes.
State and explain, using your diagram, how increasing temperature affects the rate of reaction.
Nitrosyl fluoride, NOF, can be produced by the reaction $\text{2NO(g)} + \text{F}_2\text{(g)} \rightleftharpoons \text{2NOF(g)}$. The rate is first order in NO and $\text{F}_2$. The reaction mechanism consists of two steps. Suggest equations for both steps, and state which one is the slower, rate determining step.