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JEE Main20249 Apr 2024Morning ShiftChemistryChemical KineticsActual

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 : The figure is showing "the variation in concentration against time plot" for a " (y ) " order reaction. The Value of (x+y ) is ______

Correct answer

0

Step-by-step solution

r = K [ A ]^2| ~B | if conc. are doubled aligned & r ^ = K [2 ~A ]^2[2 ~B ]^1 & r ^ =8 r x =8 aligned aligned & Zero order, y=0 & x+y=8 aligned

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