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 increase

Question

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 ______

Question diagram: Given below are two statements : Statement I: The rate law f

Answer:

8.00

Solution:

$r = K [A]^{2} ∣ B ∣$ if conc. are doubled $r^{'} = K [2 A]^{2} [2 B]^{1} r^{'} = 8 r \Rightarrow x = 8$
$\Rightarrow Zero order, y = 0 x + y = 8$

TestHub · Accepted Answer

r = K [ A ] 2 ∣ B ∣ if conc. are doubled ​ r ′ = K [ 2 A ] 2 [ 2 B ] 1 r ′ = 8 r ⇒ x = 8 ​ ​ ⇒ Zero order, y = 0 x + y = 8 ​

Chemistry - Chemical Kinetics Question with Solution | TestHub

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