If the rate of decomposition of potassium chlorate at a

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1. KClO₃ decomposes according to the reaction: 2KClO₃ → 2KCl + 3O₂
If the rate of decomposition of potassium chlorate at a certain time is determined to be 2.4 x 10^-2 mol s^-1, what is the rate of formation of KCl at the same time?

2. The rate law for a reaction involving only A and B is 1^st order in A and 4^th order in B, respectively. If the concentration of A is increased by a factor of 4 and the concentration of B is tripled the new rate will be:

3. The reaction D ---> products is first order, and the rate constant is 2.7 x 10^-4 s^-1. If the initial concentration of D is 3.00 M, then what is the final concentration of D after 1.1 hr?