1
MHT CET 2024 9th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction, $\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{(\mathrm{g})}+\mathrm{CO}_{2(\mathrm{~g})}$ rate of reaction is proportional to square of $\left[\mathrm{NO}_2\right]$ and independent of [CO]. What is the rate law equation?

A
$\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{NO}_2\right]^{\frac{1}{2}}}{[\mathrm{CO}]}$
B
$\mathrm{r}=\mathrm{k}\left[\mathrm{NO}_2\right]^2[\mathrm{CO}]^0$
C
$\mathrm{r}=\frac{1}{2} \mathrm{k}\left[\mathrm{NO}_2\right][\mathrm{CO}]$
D
$\mathrm{r}=\mathrm{k}\left[\mathrm{NO}_2\right]^2[\mathrm{CO}]$
2
MHT CET 2024 9th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

Find the percentage of unreacted reactant for zero order reaction in 90 second having rate constant $1 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$.

A
5%
B
10%
C
15%
D
20%
3
MHT CET 2024 4th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

What is the half life of a first order reaction if time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 hour?

A
1.5 hour
B
3 hour
C
6 hour
D
12 hour
4
MHT CET 2024 4th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction $2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$ rate and rate constant are $1.02 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ and $3.4 \times 10^{-5} \mathrm{~s}^{-1}$. What is the conc. of $\mathrm{N}_2 \mathrm{O}_5$ ?

A
$1.7 \mathrm{~mol} \mathrm{~L}^{-1}$
B
$3.0 \mathrm{~mol} \mathrm{~L}^{-1}$
C
$3.4 \mathrm{~mol} \mathrm{~L}^{-1}$
D
$5.1 \mathrm{~mol} \mathrm{~L}^{-1}$
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