COMEDK 2025 Afternoon Shift | Chemical Kinetics Question 10 | Chemistry

The rate constant for a zero order reaction $\mathrm{A} \rightarrow \mathrm{B}+\mathrm{C}$ is $6.0 \times 10^{-3} \mathrm{molL}^{-1} \mathrm{~s}^{-1}$. What would be the time taken for the initial concentration of A to decrease from 0.2 M to 0.024 M ?

15.83 s

37.34 s

31.90 s

29.33 s

COMEDK 2025 Morning Shift

MCQ (Single Correct Answer)

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Two statements, One Assertion (A) and the other Reason (R) are given. Choose the right option.

Assertion: The rate constant $(\mathrm{k})$ for a chemical reaction gets nearly doubled for a $10^0$ rise in temperature.

Reason: The number of bimolecular collisions between reactant molecules increase with increase in temperature

A is correct but R is wrong.

Both A and R are correct but R is not the correct explanation of A .

Both $A$ and $R$ are correct and $R$ is the correct explanation of $A$.

A is wrong but R is correct.

COMEDK 2025 Morning Shift

MCQ (Single Correct Answer)

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Two chemical reactions of the same order have equal Frequency factor value. Their Activation energies differ by $26.8 \mathrm{~kJ} / \mathrm{mol}$. At 300 K if $k_2=x k_1$ find the value of $x$.

$4.631 \times 10^4$

$1.143 \times 10^3$

$2.286 \times 10^3$

4.665

COMEDK 2025 Morning Shift

MCQ (Single Correct Answer)

-0

For a given reaction of the type $\frac{3}{5} X(a q) \rightarrow \frac{1}{2} Y(a q)+Z(g)$, the correct expression for the rate of disappearance of $X$ with reference to $Y$ is ___________

$-d \frac{[X]}{d t}=+\frac{6}{5} d \frac{[Y]}{d t}$

$-d \frac{[X]}{d t}=+\frac{5}{6} d \frac{[Y]}{d t}$

$-d \frac{[X]}{d t}=+\frac{3}{10} d \frac{[Y]}{d t}$

$-d \frac{[X]}{d t}=d \frac{[Y]^{1 / 2}}{d t}$

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