1
COMEDK 2024 Morning Shift
MCQ (Single Correct Answer)
+1
-0

The rate constant for the reaction $$\mathrm{A} \rightarrow \mathrm{B}+\mathrm{C}$$ at $$500 \mathrm{~K}$$ is given as $$0.004 \mathrm{~s}^{-1}$$. At what temperature will the rate constant become $$0.014 \mathrm{~s}^{-1}$$ ? $$\mathrm{E}_{\mathrm{a}}$$ for the reaction is $$18.231 \mathrm{~kJ}$$.

A
950 K
B
597 K
C
700 K
D
800 K
2
COMEDK 2024 Morning Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction $$\mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{NO}_{(\mathrm{g})} \rightarrow 2 \mathrm{NOCl}_{(\mathrm{g})}$$, the following data was obtained:

Experiment No. Initial concentration of $$\mathrm{Cl_2}$$ ($$\mathrm{M}$$) Initial concentration of $$\mathrm{NO}$$ ($$\mathrm{M}$$) Initial reaction rate ($$\mathrm{M}$$/min)
I 0.15 0.15 0.60
II 0.30 0.15 1.20
III 0.15 0.3 2.40
IV 0.25 0.25 2.78

Identify the order of the reaction with respect to $$\mathrm{Cl}_2, \mathrm{NO}$$ and the value of Rate constant.

A
$$\text { Order with respect to } \mathrm{Cl}_2=2 \quad \text { Order with respect to } \mathrm{NO}=1 \quad \mathrm{k}=355.5 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~min}^{-1}$$
B
$$\text { Order with respect to } \mathrm{Cl}_2=0 \quad \text { Order with respect to } \mathrm{NO}=1 \quad \mathrm{k}=8.0 \mathrm{~min}^{-1}$$
C
$$\text { Order with respect to } \mathrm{Cl}_2=1 \quad \text { Order with respect to } \mathrm{NO}=2 \quad \mathrm{k}=177.7 \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~min}^{-1}$$
D
$$\text { Order with respect to } \mathrm{Cl}_2=1 \quad \text { Order with respect to } \mathrm{NO}=1 \quad \mathrm{k}=26.66 \mathrm{~mol}^{-1} \mathrm{Lmin}^{-1}$$
3
COMEDK 2024 Morning Shift
MCQ (Single Correct Answer)
+1
-0

Given below are 4 graphs [A], [B], [C] and [D]

Identify the 2 graphs that represent a Zero order reaction?

A
[A] and [D]
B
[A] and [B]
C
[B] and [C]
D
[C] and [D]
4
COMEDK 2024 Morning Shift
MCQ (Single Correct Answer)
+1
-0

A given chemical reaction is represented by the following stoichiometric equation.

$$3 X+2 Y+\frac{5}{2} Z \rightarrow P_1+P_2+P_3$$

The rate of reaction can be expressed as _________.

A
$$\frac{2}{3}\left(\frac{d[X]}{d t}\right)=\left(\frac{d[Y]}{d t}\right)=\frac{4}{5}\left(\frac{d[Z]}{d t}\right)$$
B
$$\frac{3}{2}\left(\frac{d[X]}{d t}\right)=\frac{1}{4}\left(\frac{d[Y]}{d t}\right)=\frac{8}{5}\left(\frac{d[Z]}{d t}\right)$$
C
$$\frac{4}{15}\left(\frac{d[X]}{d t}\right)=\frac{4}{5}\left(\frac{d[Y]}{d t}\right)=\frac{8}{15}\left(\frac{d[Z]}{d t}\right)$$
D
$$\left(\frac{d[X]}{d t}\right)=\frac{3}{2}\left(\frac{d[Y]}{d t}\right)=\frac{15}{4}\left(\frac{d[Z]}{d t}\right)$$
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