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

For the reaction, $$\mathrm{A}+3 \mathrm{~B} \rightarrow 2 \mathrm{C}+\mathrm{D}$$, the concentration of $$\mathrm{A}$$ changes from 0.0150 to 0.0125 in 1 minute. The rate of formation of $$\mathrm{C}$$ in $$\mathrm{mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$$ is:

A
$$6.32 \times 10^{-5}$$
B
$$8.32 \times 10^{-5}$$
C
$$3.26 \times 10^{-5}$$
D
$$2.5 \times 10^{-5}$$
2
COMEDK 2024 Afternoon Shift
MCQ (Single Correct Answer)
+1
-0

The rate of appearance of bromine is related to the disappearance of bromide ion in the equation given below is:

$$\mathrm{BrO}_3^{-} \text {(aq) }+5 \mathrm{Br}^{-} \text {(aq) }+6 \mathrm{H}^{+} \rightarrow 3 \mathrm{Br}_2(\mathrm{l})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})$$

A
$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=\frac{5}{3} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$
B
$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=-\frac{1}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$
C
$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=\frac{3}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$
D
$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=-\frac{3}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$
3
COMEDK 2024 Afternoon Shift
MCQ (Single Correct Answer)
+1
-0

The half-life for a zero order reaction is

A
Inversely proportional to the initial concentration and directly proportional to the rate constant
B
Directly proportional to the initial concentration and inversely proportional to the rate constant
C
Independent of rate constant, but depends on the initial concentration
D
Independent of initial concentration
4
COMEDK 2024 Morning Shift
MCQ (Single Correct Answer)
+1
-0

The time required for $$80 \%$$ of a first order reaction is "$$y$$" times the half-life period of the same reaction. What is the value of "$$y$$"?

A
3.22
B
2.32
C
0.322
D
2.96
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