Explain why this reaction is a redox reaction using oxidation numbers.
Nitrosyl bromide has a trivalent nitrogen atom. Draw the ‘dot-and-cross’ diagram for NOBr. Show only outer electrons.
The reaction rate was measured at a range of concentrations of the two reactants, NO and $\text{Br}_2$, and the results below were obtained. The general rate equation for this reaction is written as: rate $= k[\text{NO}]^{a}[\text{Br}_2]^{b}$.
What does the term order of reaction with respect to a particular reagent mean?
Use the data in the table to deduce the values of $a$ and $b$ in the rate equation. Show your working.
Use the table data to calculate the initial rate for experiment 4.
Use the results from experiment 1 to calculate the rate constant, $k$, for this reaction. Include the units for $k$.
Using the rate equation, explain why the rate falls as temperature decreases.
The reaction between X and Y was investigated: $\text{2X} + \text{Y} \rightarrow \text{Z}$. A possible mechanism is shown below. step 1: $\text{2X} \rightarrow \text{V}$; step 2: $\text{V} + \text{Y} \rightarrow \text{Z}$. The general rate equation for this reaction is written as: rate $= k[\text{X}]^{m}[\text{Y}]^{n}$. Step 1 is the slower step in the mechanism. Deduce the values of $m$ and $n$ in the rate equation.