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1
MHT CET 2025 20th April Morning Shift
MCQ (Single Correct Answer)
+1
-0

Which of the following equations is correct regarding rate of disappearance of reactant and appearance of product for

$$ \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})} $$

A

$3 \frac{\mathrm{~d}\left[\mathrm{~N}_2\right]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{~d}\left[\mathrm{~N}_2\right]}{\mathrm{dt}}$

B

$\frac{1}{2} \frac{\mathrm{~d}\left[\mathrm{~N}_2\right]}{\mathrm{dt}}=\frac{1}{3} \frac{\mathrm{~d}\left[\mathrm{H}_2\right]}{\mathrm{dt}}$

C

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

D

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

2
MHT CET 2025 19th April Evening Shift
MCQ (Single Correct Answer)
+1
-0

Which from following is a correct representation of reaction rate for reaction stated below?

$$ \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{NH}_{3(\mathrm{~g})} $$

A

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

B

$\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{dt}}=-\frac{1}{3} \frac{\mathrm{~d}\left[\mathrm{H}_2\right]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{~d}\left[\mathrm{NH}_3\right]}{\mathrm{dt}}$

C

$-\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{dt}}=-\frac{1}{3} \frac{\mathrm{~d}\left[\mathrm{H}_2\right]}{\mathrm{dt}}=\frac{\mathrm{1}}{2} \frac{\mathrm{~d}\left[\mathrm{NH}_3\right]}{\mathrm{dt}}$

D
$\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{dt}}=\frac{1}{3} \frac{\mathrm{~d}\left[\mathrm{H}_2\right]}{\mathrm{dt}}=-\frac{1}{2} \frac{\mathrm{~d}\left[\mathrm{NH}_3\right]}{\mathrm{dt}}$
3
MHT CET 2025 19th April Evening Shift
MCQ (Single Correct Answer)
+1
-0

Half life of a first order reaction is 900 minute at 400 K , find its half life at 300 K ?

$$ \left(\frac{\mathrm{E}_{\mathrm{a}}}{2.303 \mathrm{R}}=1.3056 \times 10^3\right) $$

A
5512.5 minute
B
11025.0 minute
C
8314.3 minute
D
2303.1 minute
4
MHT CET 2025 19th April Evening Shift
MCQ (Single Correct Answer)
+1
-0

Rate law for the reaction,

$$ \mathrm{C}_2 \mathrm{H}_5 \mathrm{I}_{(\mathrm{g})} \longrightarrow \mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{HI}_{(\mathrm{g})} \text { is } \mathrm{r}=\mathrm{k}\left[\mathrm{C}_2 \mathrm{H}_5 \mathrm{I}\right] $$

What is the order and molecularity of this reaction?

A
order and molecularity both are 1
B
order is 1 and molecularity is 2
C
order and molecularity both are 2
D
order is 2 and molecularity is 1
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