1. For a reaction of the type A + B + C
going to products, the following observations are made: doubling
the concentration of A has no effect on the rate, doubling the
concentration of B increases the rate by a factor of 4, and
tripling the concentration of C triples the rate. What is the rate
law for the reaction?
2. A first order reaction has a half-life
of 5 minutes. If the initial concentration of reactant is 0.80 M,
what will its concentration be after 15 minutes?
3. The following mechanism is proposed for
a chemical reaction:
i) B + B --> B2
slow
ii) B2 + A --> AB + B
fast
What rate law does this mechanism suggest for this reaction?
Please explain/ show working out