Nitric oxide and oxygen react according to the equation:
2NO(g)+O2(g)→2NO2(g) 2\text{NO}(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\text{NO}_2(\text{g}) 2NO(g)+O2(g)→2NO2(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[O2] \text{rate} = k [\text{NO}]^2[\text{O}_2] rate=k[NO]2[O2]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 [O2][\text{O}_2][O2] / 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 | 0.400.400.40 | 2.0×10−22.0 \times 10^{-2}2.0×10−2 |
| 2 | 0.400.400.40 | 4.5×10−24.5 \times 10^{-2}4.5×10−2 | |
| 3 | 0.400.400.40 | 0.800.800.80 | |
| 4 | 0.100.100.10 | 5.0×10−35.0 \times 10^{-3}5.0×10−3 |
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.
