Nitrogen monoxide and chlorine react according to the equation:
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)A series of experiments was carried out at a given temperature to study this reaction. The results were used to deduce the rate equation:
rate=k[NO]2[Cl2] \text{rate} = k [\text{NO}]^2[\text{Cl}_2] rate=k[NO]2[Cl2]Table 1 shows an incomplete set of experimental results.
Table 1
| Experiment | Initial [NO][\text{NO}][NO] / mol dm−3\text{mol dm}^{-3}mol dm−3 | Initial [Cl2][\text{Cl}_2][Cl2] / mol dm−3\text{mol dm}^{-3}mol dm−3 | Initial rate of reaction / mol dm−3 s−1\text{mol dm}^{-3}\text{ s}^{-1}mol dm−3 s−1 |
|---|---|---|---|
| 1 | 0.200.200.20 | 0.300.300.30 | 5.4×10−25.4 \times 10^{-2}5.4×10−2 |
| 2 | 0.300.300.30 | 2.16×10−12.16 \times 10^{-1}2.16×10−1 | |
| 3 | 0.400.400.40 | 0.600.600.60 | |
| 4 | 0.100.100.10 | 9.0×10−39.0 \times 10^{-3}9.0×10−3 |
Use the data from Experiment 1 to calculate a value for the rate constant, kkk, at this temperature and state its units. Give your answer to an appropriate number of significant figures.
Complete Table 1 by calculating the missing initial concentrations and initial rate.
