15. Chemical Kinetics
Reaction Mechanism
15. Chemical Kinetics Reaction Mechanism
4PRACTICE PROBLEM
The rate of the decomposition of hydrogen peroxide is directly proportional to the concentration of H2O2 and Pt (Rate = k [H2O2] [Pt]). Shown below is the reaction mechanism.
Step 1. Pt + H2O2 → H2O + Pt(O) (slow)
Step 2. Pt(O) + H2O2 → Pt + O2 + H2O (fast)
Overall equation: 2 H2O2 → O2 + H2O
Explain why Pt is in the rate law but is not in the overall chemical equation.
The rate of the decomposition of hydrogen peroxide is directly proportional to the concentration of H2O2 and Pt (Rate = k [H2O2] [Pt]). Shown below is the reaction mechanism.
Step 1. Pt + H2O2 → H2O + Pt(O) (slow)
Step 2. Pt(O) + H2O2 → Pt + O2 + H2O (fast)
Overall equation: 2 H2O2 → O2 + H2O
Explain why Pt is in the rate law but is not in the overall chemical equation.