CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

For a reactions $$A+B\rightarrow product$$, it was found that rate of reaction increases four times if concentration of 'A' is doubled, but the rate of reaction remains unaffected, if concentration of 'B' is doubled. Hence, the rate law for the reaction is:

 $$[MP PET/PMT 1998; MP PMT 2003]$$


A
rate=k[A][B]
loader
B
rate=k[A]2
loader
C
rate=k[A]2[B]1
loader
D
rate=k[A]2[B]2
loader

Solution

The correct option is C $$rate=k\left[A\right]^{2}$$
Let the rate of reaction depends on $$x$$ power of $$\left[A\right]$$. 

Then
$$r_{1}=k\left[A\right]^{x}$$ and $$r_{2}=k\left[2A\right]^{x}$$
$$\therefore\dfrac{r_1}{r_2}=\dfrac{\left[A\right]^{x}}{\left[2A\right]^{x}}=\dfrac{1}{4}=\left(\dfrac{1}{2}\right)^{2} \, \, \,\left(\because{r_{2}=4r_1}\right)$$

$$\therefore{x=2}$$, As the reaction rate does not depend upon the concentration of $$B$$. 

Hence, the correct rate law will be $$rate=K\left[A\right]^{2}\left[B\right]^{o}$$ or $$=K\left[A\right]^{2}$$

Chemistry
NCERT
Standard XII

Suggest Corrections
thumbs-up
 
0


similar_icon
Similar questions
View More


similar_icon
Same exercise questions
View More


similar_icon
People also searched for
View More



footer-image