An inorganic chemistry researcher studies the kinetics of the following reaction in aqueous solution at a constant temperature of 298 K298\text{ K}298 K:
P(aq)+2Q(aq)+2R(aq)→S(aq)+2T(aq) \text{P}(\text{aq}) + 2\text{Q}(\text{aq}) + 2\text{R}(\text{aq}) \rightarrow \text{S}(\text{aq}) + 2\text{T}(\text{aq}) P(aq)+2Q(aq)+2R(aq)→S(aq)+2T(aq)The researcher measures the initial rate of reaction across four experiments with varying initial concentrations of the reactants. The results are summarized in the table below:
| Experiment | [P][\text{P}][P] / mol dm−3\text{mol dm}^{-3}mol dm−3 | [Q][\text{Q}][Q] / mol dm−3\text{mol dm}^{-3}mol dm−3 | [R][\text{R}][R] / mol dm−3\text{mol dm}^{-3}mol dm−3 | Initial rate / mol dm−3 s−1\text{mol dm}^{-3}\text{ s}^{-1}mol dm−3 s−1 |
|---|---|---|---|---|
| 1 | 2.00 × 10-2 | 1.50 × 10-2 | 1.00 × 10-2 | 3.60 × 10-6 |
| 2 | 2.00 × 10-2 | 3.00 × 10-2 | 1.00 × 10-2 | 1.44 × 10-5 |
| 3 | 2.00 × 10-2 | 3.00 × 10-2 | 3.00 × 10-2 | 1.44 × 10-5 |
| 4 | 4.00 × 10-2 | 1.50 × 10-2 | 2.00 × 10-2 | 7.20 × 10-6 |
Explain how the reaction order with respect to each reactant can be determined from these results. Hence, determine the rate equation and the rate constant (including units) for this reaction.
