Given below are two statements : Statement I : The rate law for the reaction A + B C is rate (r) = k[A]2[B]. When the concentration of both A and B is doubled, the reaction rate is increased “x” times

Question

Given below are two statements : Statement I : The rate law for the reaction A + B C is rate (r) = k[A]2[B]. When the concentration of both A and B is doubled, the reaction rate is increased “x” times. Statement II : Time Contration of R o [Ro] –K = Slope The figure is showing “the variation in concentration against time plot” for a “y” order reaction. The value of x + y is ______________.

Prashant Kotian · Accepted Answer

Correct answer: .. r = K[A]2|B| if conc. are doubled r' = K[2A]2[2B]1 r' = 8r  x = 8 C t –K   Zero order, y = 0 x + y = 8

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