Chemical Kinetics

A drug becomes ineffective when it decomposes to 50 % its concentration. If 16 mg of said drug becomes 4 mg in 12 months, find the time in which drug becomes ineffective given that decomposition of drug follows first order kinetics.

Memory Based Question 29/Jan/25 Evening shift

The rate of a reaction quadruples when temperature changes from \(27^\circ C\) to \(57^\circ C\). Calculate the energy of activation.
Given \(R=8.314J{K}^{-1}mo{l}^{-1},\log 4=0.6021\)

[NEET 2024]

For an elementary reaction

\(\mathrm{A}+\mathrm{B}\to \mathrm{C}+\mathrm{D}\)

When volume becomes \(\frac{1}{3}\)rd, rate of reaction becomes:

The reaction \({A}_{2}+{B}_{2}\to 2AB\) follows the mechanism

\({A}_{2}\overset{{k}_{1}}{\underset{{k}_{-1}}{⇌}}A+A\text{ (fast) }\\ A+{B}_{2}\overset{{k}_{2}}{\to }AB+B\text{ (slow) }\\ A+B\to AB\text{ (fast) }\)

The overall order of the reaction is

Activation energy of any chemical reaction can be calculated if one knows the value of

[NEET 2024]

Which of the following statement is not true for radioactive decay?

[JEE Main 2025, 22 Jan (Shift 1)]

If for a first-order reaction, the value of A and \({E}_{a}\) are \(4\times {10}^{13}{s}^{-1}\)and 98.6 kJ \(mo{l}^{-1}\)respectively, then at what temperature will its half-life be 10 minutes?

Find the order of the reaction

\(\mathrm{A}+\mathrm{B}\to \mathrm{F}\)

if the mechanism of the reaction is given below:
Step 1: \(\mathrm{A}+\mathrm{B}\to \mathrm{D}(\mathrm{slow})\)
Step 2: \(\mathrm{D}\to \mathrm{C}+\mathrm{E}(\mathrm{fast})\)
Step 3: \(\mathrm{C}+\mathrm{E}\to \mathrm{F}(\mathrm{fast})\)

Memory Based Question 29/Jan/25 Morning shift

Drug X becomes ineffective after 50% decomposition. The original concentration of drug in a bottle was 16 mg / mL which becomes 4 mg / mL in 12 months. The expiry time of the drug in months is ______.
Assume that the decomposition of the drug follows first order kinetics

[JEE Main 2025, 29 Jan (Shift 2)]

Consider an elementary reaction

\(A(g)+B(g)\to C(g)+D(g)\)

If the volume of reaction mixture is suddenly reduced to \(\frac{1}{3}\) of its initial volume, the reaction rate will become ' x ' times of the original reaction rate. The value of x is:

[JEE Main 2025, 28 Jan (Shift 2)]

For a first order reaction, the time required for completion of 90% reaction is 'x' times the half life of the reaction. The value of 'x' is:

(Given: In 10 = 2.303 and log 2 = 0.3010)

For a certain reaction, the rate \(=\mathrm{k}[\mathrm{A}{]}^{2}[\mathrm{B}]\), when the initial concentration of A is tripled keeping concentration of B constant, the initial rate would: