1
MHT CET 2019 2nd May Evening Shift
MCQ (Single Correct Answer)
+1
-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

A
$3.2 \times 10^{-6} \mathrm{~s}^{-1}$
B
zero
C
$1.6 \times 10^{-6} \mathrm{~s}^{-1}$
D
$1.6 \times 10^{-5} \mathrm{~s}^{-1}$
2
MHT CET 2019 2nd May Evening Shift
MCQ (Single Correct Answer)
+1
-0

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

A
increases by a factor of 8
B
increases by a factor of 4
C
increases by a factor of 3
D
increases by a factor of 2
3
MHT CET 2019 2nd May Evening Shift
MCQ (Single Correct Answer)
+1
-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

A
homogenous catalyst
B
acid catalyst
C
heterogenous catalyst
D
enzyme catalyst
4
MHT CET 2019 2nd May Morning Shift
MCQ (Single Correct Answer)
+1
-0

For the elementary reaction $2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_3(g)$, identify the correct among the following relations

A
$\frac{-d\left[\mathrm{SO}_2(g)\right]}{d t}=\frac{-d\left[\mathrm{O}_2(g)\right]}{d t}$
B
$\frac{+1}{2} \frac{d\left[\mathrm{SO}_3(g)\right]}{d t}=\frac{d\left[\mathrm{SO}_2(g)\right]}{d t}$
C
$\frac{+d\left[\mathrm{SO}_3(g)\right]}{d t}=\frac{-2 d\left[\mathrm{O}_2(g)\right]}{d t}$
D
$\frac{+d\left[\mathrm{SO}_2(g)\right]}{d t}=\frac{-d\left[\mathrm{O}_2(g)\right]}{d t}$
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