1
MHT CET 2024 15th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

A first order reaction takes 40 minute for $20 \%$ decomposition. Calculate its rate constant.

A
$5.6 \times 10^{-3}$ minute $^{-1}$
B
$4.5 \times 10^{-3}$ minute $^{-1}$
C
$6.5 \times 10^{-3}$ minute ${ }^{-1}$
D
$7.2 \times 10^{-3}$ minute $^{-1}$
2
MHT CET 2024 11th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

If instantaneous rate of reaction is given as $$ -\frac{1}{\mathrm{a}} \frac{\mathrm{~d}[\mathrm{~A}]}{\mathrm{dt}}=-\frac{1}{\mathrm{~b}} \frac{\mathrm{~d}[\mathrm{~B}]}{\mathrm{dt}}=\frac{1 \mathrm{~d}[\mathrm{C}]}{\mathrm{c}]}=\frac{1 \mathrm{~d}[\mathrm{D}]}{\mathrm{d}]}$$

the reaction is represented as

A
$\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D}$
B
$\mathrm{aA}+\mathrm{B} \longrightarrow \mathrm{cC}+\mathrm{dD}$
C
$\mathrm{aA}+\mathrm{bB} \longrightarrow \mathrm{cC}+\mathrm{dD}$
D
$\mathrm{aA}+\mathrm{bB} \longrightarrow \mathrm{C}+\mathrm{D}$
3
MHT CET 2024 11th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

Rate law for a reaction is $r=k[A]^2[B]$. If rate constant is $6.25 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{~s}^{-1}$, what is the rate of reaction when $[\mathrm{A}]=1 \mathrm{~mol} \mathrm{dm}^{-3}$ and $[\mathrm{B}]=0.2 \mathrm{~mol} \mathrm{dm}^{-3}$ ?

A
$1.250 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$
B
$2.125 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$
C
$3.105 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$
D
$2.0 \times 10^{-2} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$
4
MHT CET 2024 11th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

What is the time needed to reduce the initial concentration of reactant to $10 \%$ in a first order reaction if its half life time is 10 minutes?

A
15 minute
B
20 minute
C
25 minute
D
33 minute
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