MHT CET 2019 3rd May Morning Shift | Chemical Kinetics Question 76 | Chemistry

For the elementary reaction, $3 \mathrm{H}_2(g)+\mathrm{N}_2(g) \longrightarrow 2 \mathrm{NH}_3(g)$ identify the correct relation among the following relations:

$\frac{-3}{2} \frac{d\left[\mathrm{H}_2(\mathrm{~g})\right]}{d t}=\frac{d\left[\mathrm{NH}_3(\mathrm{~g})\right]}{d t}$

$\frac{-2}{3} \frac{d\left[\mathrm{H}_2(\mathrm{~g})\right]}{d t}=\frac{d\left[\mathrm{NH}_3(\mathrm{~g})\right]}{\mathrm{dt}}$

$\frac{d\left[\mathrm{NH}_3(g)\right]}{d t}=\frac{-1}{3} \frac{d\left[H_2(g)\right]}{d t}$

$\frac{-d\left[H_2(g)\right]}{d t}=\frac{d\left[\mathrm{NH}_3(g)\right]}{d t}$

MHT CET 2019 2nd May Evening Shift

MCQ (Single Correct Answer)

-0

The activation energy of a reaction is zero. Its rate constant at 280 K is $1.6 \times 10^{-6} \mathrm{~s}^{-1}$, the rate constant at 300 K is

$3.2 \times 10^{-6} \mathrm{~s}^{-1}$

zero

$1.6 \times 10^{-6} \mathrm{~s}^{-1}$

$1.6 \times 10^{-5} \mathrm{~s}^{-1}$

MHT CET 2019 2nd May Evening Shift

MCQ (Single Correct Answer)

-0

For a chemical reaction rate law is, rate $=k[A]^2[B]$. If $[A]$ is doubled at constant $[B]$, the rate of reaction

increases by a factor of 8

increases by a factor of 4

increases by a factor of 3

increases by a factor of 2

MHT CET 2019 2nd May Evening Shift

MCQ (Single Correct Answer)

-0

In the reaction, $\mathrm{H}_2 \mathrm{O}_2(a q) \xrightarrow{\mathrm{I_{(aq)}^-}} \mathrm{H}_2 \mathrm{O}(I)+\frac{1}{2} \mathrm{O}_2(g)$ iodide ion acts as

homogenous catalyst

acid catalyst

heterogenous catalyst

enzyme catalyst

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