The rate of a reaction A + 2B → P is 2 × 10−2 M/ min, when concentrations of each A and B are 1.0 M.

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The rate of a reaction A + 2B → P is 2 × 10−2 M/ min, when concentrations of each A and B are 1.0 M. If the rate of reaction r = K[A]2[B], the rate of reaction when half of the B has reacted should be

Accepted Answer

A + 2B ? Pt1 1.0 M 1.0 Mt2 1.0 – 0.25 1.0 – 0.5= 0.75 M = 0.5 MNow, $\frac{r_{2}}{r_{1}} = \frac{K\left\lbrack A_{2} ightbrack^{2}\left\lbrack B_{2} ightbrack}{K\left\lbrack A_{1} ightbrack^{2}\left\lbrack B_{1} ightbrack} \Rightarrow \frac{r_{2}}{2 	imes 10^{- 2}} = \frac{(0.75)^{2} 	imes 0.5}{(1.0)^{2} 	imes 1.0}$$	herefore r_{2} = 5.625 	imes 10^{- 3}	ext{ M/min}$

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