Notes
1. Clock Reaction (Initial rate method)
1.5. Procedure to determine the order of reaction with respect to S2O3(2-) ions
Experiment | \([H^+]\) / mol dm\(^{-3}\) | \(\text{S}_2\text{O}_3^{2-}\) / mol dm\(^{-3}\) | Time (s) |
1 | 0.001 | 0.001 | 120 |
2 | 0.001 | 0.002 | 60 |
Calculate Rate of Reaction
Experiment | \([H^+]\) / mol dm\(^{-3}\) | \(\text{S}_2\text{O}_3^{2-}\) / mol dm\(^{-3}\) | Time (s) | Rate of Reaction (1/time) |
1 | 0.001 | 0.001 | 120 | \( \frac{1}{120} \approx 0.0083 \) s\(^{-1}\) |
2 | 0.001 | 0.002 | 60 | \( \frac{1}{60} \approx 0.0167 \) s\(^{-1}\) |
W.r.t S2O32− and H+
Compare Expt 1 and Expt 2 where [H+] is the same.
When \([\text{S}_2\text{O}_3^{2-}]_{\text{Expt 2}}\) is twice of
\([\text{S}_2\text{O}_3^{2-}]_{\text{Expt 1}}\)
o Rate (2) is twice of rate (1)
o Order w.r.t \(\text{S}_2\text{O}_3^{2-}\) is one.