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For the reaction, $$2A + B \rightarrow$$ Products, when the concentrations of $$A$$ and $$B$$ both were doubled, the rate of the reaction increased from $$0.3\text{ mol L}^{-1}\text{ s}^{-1}$$ to $$2.4\text{ mol L}^{-1}\text{ s}^{-1}$$. When the concentration of $$A$$ alone is doubled, the rate increased from $$0.3\text{ mol L}^{-1}\text{ s}^{-1}$$ to $$0.6\text{ mol L}^{-1}\text{ s}^{-1}$$.<br>Which one of the following statements is correct?
Let rate $$= k[A]^m[B]^n$$. Doubling $$A$$ alone doubles the rate, so $$2^m = 2$$ and $$m = 1$$. Doubling both multiplies the rate by $$\frac{2.4}{0.3} = 8$$, so $$2^{m + n} = 8$$ and $$n = 2$$. So the order with respect to $$B$$ is 2 (total order 3).
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