COMEDK 2024 Afternoon Shift | Chemical Kinetics Question 33 | Chemistry

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:

$$6.32 \times 10^{-5}$$

$$8.32 \times 10^{-5}$$

$$3.26 \times 10^{-5}$$

$$2.5 \times 10^{-5}$$

COMEDK 2024 Afternoon Shift

MCQ (Single Correct Answer)

-0

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

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

$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=\frac{5}{3} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$

$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=-\frac{1}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$

$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=\frac{3}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$

$$ \frac{\mathrm{d}\left[\mathrm{Br}_2\right]}{\mathrm{dt}}=-\frac{3}{5} \frac{\mathrm{d}\left[\mathrm{Br}^{-}\right]}{\mathrm{dt}} $$

COMEDK 2024 Afternoon Shift

MCQ (Single Correct Answer)

-0

The half-life for a zero order reaction is

Inversely proportional to the initial concentration and directly proportional to the rate constant

Directly proportional to the initial concentration and inversely proportional to the rate constant

Independent of rate constant, but depends on the initial concentration

Independent of initial concentration

COMEDK 2024 Morning Shift

MCQ (Single Correct Answer)

-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 "$$y$$"?

3.22

2.32

0.322

2.96

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