1. After 45.0 min, 43.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics?
2. Consider the following mechanism.
step 1: A + B -> C slow
step 2: A + C -> D fast
overall: 2A + B -> D
Determine the rate law for the overall reaction (where the overall rate constant is represented as k).
3. The following reaction has an activation energy of 262 kJ/mol.
C4H8(g) -> 2C2H4(g)
At 600.0 K the rate constant is 6.1� 10�8 s�1. What is the value of the rate constant at 780.0 K?
4. Consider this initial-rate data at a certain temperature for the reaction described by
C2H5Cl(g) -> C2H4(g) + HCl(g)
Determine the value and units of the rate constant.
[C2H5Cl]0 (M) Initial Rate (M/s)
0.100 = 0.805×10^-30
0.200 = 1.61×10^-30
0.300 = 2.42×10^-30
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