JEE-Main 2019_CK_9-1-19_S2 - Competishun – Live JEE & NEET Courses and Exam Prep

JEE MAIN 2019

09-01-19 S2

Question

For the reaction, $2 \mathrm{~A}+\mathrm{B} \rightarrow$ products, when the concentration of A and B both were doubled, the rate of the reaction increased from $0.3 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ to $2.4 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$. When the concentration of A alone is doubled, the rate increased from $0.3 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ to $0.6 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$. Which one of the following statements is correct

Select the correct option:

Order of the reaction with respect to A is 2

Order of the reaction with respect to B is 1

Order of the reaction with respect to B is 2

Total order of the reaction is 4

✓ Correct! Well done.

✗ Incorrect. Try again or view the solution.

Solution

$\begin{aligned} & r=K[A]^x[B]^y \\ & \frac{r_2}{r_1}=2^x \cdot 2^y=8 \Rightarrow x+y=3 \\ & \frac{r_3}{r_1}=2^x=2 \Rightarrow x=1 \\ & \therefore y=2\end{aligned}$

Question Tags

JEE Main

Chemistry

Easy

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