Question

the overall order of reaction between X and Y is 3. which of the following rate equation must be correct, if on doubling the concentration of X, the rate of reactions gets doubled?
(1) K [X]^2 [Y]^0
(2) K [X]^1 [Y]^2
(3) K [X]^1 [Y]^3

Answer 1

Answer: The correct answer is option 2.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$Rate=k[X]^x[Y]^y$

k= rate constant

x = order with respect to X

y = order with respect to Y

n = x+y = Total order = 3

According to the question:

$Rate_1=k[X]^x[Y]^y$

and

$2\times Rate_1=k[2X]^x[Y]^y$

Taking the ratio of two rates, we get:

$\frac{2\times Rate_1}{Rate_1}=\frac{k[2X]^x[Y]^y}{k[X]^x[Y]^y}\\\\2=2^x\\\\x=1$

As, total order of the reaction is 3, so

$x+y=3\\y=3-1\\y=2$

so, the rate equation becomes:

$Rate=k[X]^1[Y]^2$

Hence, the correct answer is Option 2.

Answer 2

Answer:

option 2 i e r = [x]^1 [y]^2

Explanation:

just see the uploaded photo