JEE Main · 2024 · 09 Apr 2024 · Shift 1 · Chemical Kinetics

Given below are two statements :

Statement I : The rate law for the reaction

A + B \to 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 ______.

Answer: 8

Solution

Rate

= k [A]^{2} [B]

; doubling both multiplies the rate by

2^{2} \cdot 2 = 8

, so

x = 8

. The straight-line concentration-vs-time plot means zero order,

y = 0

x + y = 8

JEE Main · 2024 · 09 Apr 2024 · Shift 1 · Integer answer

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