1
MHT CET 2024 11th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

Rate constant of a reaction, $$ 2 \mathrm{NO}_2 \mathrm{Cl}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}$$

is 4.7672 minute $^{-1}$. Calculate half life of reaction.

A
0.0727 minute
B
0.1454 minute
C
0.2181 minute
D
0.4362 minute
2
MHT CET 2024 11th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

Initial concentration of reactant in a first order reaction is $0.08 \mathrm{~mol} \mathrm{~dm}^{-3}$ What concentration would remain after 40 minute?

$$\left(\text { given } \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}=5.00\right)$$

A
$0.008 \mathrm{~mol} \mathrm{~dm}^{-3}$
B
$0.08 \mathrm{~mol} \mathrm{~dm}^{-3}$
C
$0.016 \mathrm{~mol} \mathrm{~dm}^{-3}$
D
$0.032 \mathrm{~mol} \mathrm{~dm}^{-3}$
3
MHT CET 2024 10th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction $\mathrm{A}+\mathrm{B} \longrightarrow$ product, rate law equation is, rate $=k[A]^2[B]$. If rate of reaction is $0.22 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$, calculate rate constant. ($\mathrm{[A}]=1 \mathrm{~mol} \mathrm{~L}^{-1},[\mathrm{~B}]=0.25 \mathrm{~mol} \mathrm{~L}^{-1})$

A
$0.44 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$
B
$0.88 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$
C
$1.136 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$
D
$3.52 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$
4
MHT CET 2024 10th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

Rate of a first order reaction is $1.5 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1}$ minute ${ }^{-1}$ at 0.5 M concentration of reactant, calculate half life of reaction.

A
0.383 minute
B
7.53 minute
C
8.73 minute
D
23.1 minute
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