| Sections | |||
|---|---|---|---|
| Rate of Reaction | 11 mins | 0 completed | Learn Summary |
| Average Rate of Reaction | 18 mins | 0 completed | Learn |
| Arrhenius Equation | 16 mins | 0 completed | Learn Summary |
| Rate Law | 38 mins | 0 completed | Learn Summary |
| Integrated Rate Law | 52 mins | 0 completed | Learn Summary |
| Collision Theory | 9 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Instantaneous Rate of Change |
| Energy Diagram |
| Catalyst |
| Michaelis-Menten Equation |
| Reaction Mechanism |
| Identifying Reaction Order |
The decomposition of N2O5 can be described by the equation
2N2O5 → 4NO2 + O2
Given these data for the reaction at 45 °C in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval.
t(s) [N2O5]
0 2.04
135 1.87
536 1.46
795 1.24
i) Reaction rate from 0-135 is ?
ii) Reaction rate from 135-536 is ?
iii) Reaction rate from 536-795 is ?
Average rate = Δ[ N2O5 ] / 2Δt
Because we lose reactants and gain products, we are losing [N2O5], and our equation becomes:
Average rate = - Δ[ N2O5 ] / 2Δt
Also, remember that Δ[ N2O5 ] and Δt = final - initial, and that whatever the coefficient we have for the reactant, we will put that number on the bottom!
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