Question: Which of the following is not a first order reaction?
A Decomposition of H2O2
B Decomposition of N2O
C Decomposition of N2O5
D Decomposition of SO2Cl2
Answer: Decomposition of N2O
| Aspect | Description |
| Reaction Order | First order |
| Rate Law Expression | A → Products
Rate = k[A] where [A] is the concentration of reactant A |
| Rate Constant (k) | Positive constant that depends on the specific reaction |
| Dependence on Concentration | The rate of the reaction is directly proportional to the concentration of the reactant (A) |
| Half-life | t1/2 = (0.693 / k) |
| Units of Rate Constant (k) | Depends on the overall reaction order |
| Examples
|
· Decomposition of SO2Cl2
SO2Cl2 → Cl2 + SO2 Rate = k[SO2Cl2] · Decomposition of N2O5 2N2O5 → O2 + 4NO2 Rate = k[N2O5] · Decomposition of H2O2 2H2O2 → 2H2O + O2 Rate = k[H2O2] |