## 7B.9

$\frac{d[R]}{dt}=-k[R]; \ln [R]=-kt + \ln [R]_{0}; t_{\frac{1}{2}}=\frac{0.693}{k}$

RRahimtoola1I
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### 7B.9

How do you do this problem or other problems similar to this when they give you only the initial concentration of the reactant and then a later concentration of a product?

For the first-order reaction A > 3B + C, when initial concentration of A = 0.015 mol/L, the concentration of B increases to 0.018 mol/L in 3.0 min. (a) What is the rate constant for the reaction expressed as the rate of loss of A? (b) How much more time would be needed for the concentration of B to increase to 0.030 mol/L?