An oxide of nitrogen and chlorine react to form nitrosyl chloride:
2NO(g)+Cl2(g)→2NOCl(g) 2\text{NO}(\text{g}) + \text{Cl}_2(\text{g}) \rightarrow 2\text{NOCl}(\text{g}) 2NO(g)+Cl2(g)→2NOCl(g)Explain how increasing the temperature increases the rate of this reaction. In your answer, describe what a labelled sketch using Boltzmann distributions would show (stating the labels for both axes and how the distribution curve changes with a temperature increase).
The rate of this reaction is investigated by carrying out three experiments at the same temperature. The results are shown in the table below:
| Experiment | [NO(g)] / mol dm−3[\text{NO}(\text{g})] \ / \ \text{mol dm}^{-3}[NO(g)] / mol dm−3 | [Cl2(g)] / mol dm−3[\text{Cl}_2(\text{g})] \ / \ \text{mol dm}^{-3}[Cl2(g)] / mol dm−3 | Initial rate / mol dm−3s−1\ / \ \text{mol dm}^{-3}\text{s}^{-1} / mol dm−3s−1 |
|---|---|---|---|
| 1 | 1.50 × 10-3 | 2.00 × 10-3 | 1.20 × 10-3 |
| 2 | 3.00 × 10-3 | 2.00 × 10-3 | 4.80 × 10-3 |
| 3 | 6.00 × 10-3 | 8.00 × 10-3 | 7.68 × 10-2 |
Determine the orders with respect to NO\text{NO}NO and Cl2\text{Cl}_2Cl2, the rate equation, and the value of the rate constant, kkk, including its units. Explain your reasoning.
Nitryl chloride decomposes according to the following equation:
2NO2Cl(g)→2NO2(g)+Cl2(g) 2\text{NO}_2\text{Cl}(\text{g}) \rightarrow 2\text{NO}_2(\text{g}) + \text{Cl}_2(\text{g}) 2NO2Cl(g)→2NO2(g)+Cl2(g)The rate equation for this reaction is:
rate=k[NO2Cl(g)] \text{rate} = k[\text{NO}_2\text{Cl}(\text{g})] rate=k[NO2Cl(g)]Suggest a possible two-step mechanism for this reaction, where the first step is much slower than the second step.
