NVAMediumJEE 2023Integrated Rate Laws

JEE Chemistry 2023 Question with Solution

A and B are two substances undergoing radioactive decay in a container. The half-life of A is 15min15 \, \text{min} and that of B is 5min5 \, \text{min}. If the initial concentration of B is 44 times that of A and they both start decaying at the same time, how much time will it take for the concentration of both of them to be same? _____ min\text{min}.

Answer

Correct answer:15

Step-by-step solution

Standard Method

Given: Half-life of A is 15min15 \, \text{min}, half-life of B is 5min5 \, \text{min}, and initial concentration of B is 44 times that of A.

Find: The time when concentrations of A and B become equal.

The decay of a substance follows:

N(t)=N0×(12)t/t1/2N(t) = N_0 \times \left(\frac{1}{2}\right)^{t/t_{1/2}}

Let the initial concentration of A be NAN_A. Then the initial concentration of B is NB=4NAN_B = 4N_A.

For substance A:

NA(t)=NA×(12)t/15N_A(t) = N_A \times \left(\frac{1}{2}\right)^{t/15}

For substance B:

NB(t)=4NA×(12)t/5N_B(t) = 4N_A \times \left(\frac{1}{2}\right)^{t/5}

At the required time, concentrations are equal:

NA×(12)t/15=4NA×(12)t/5N_A \times \left(\frac{1}{2}\right)^{t/15} = 4N_A \times \left(\frac{1}{2}\right)^{t/5}

Cancel NAN_A from both sides:

(12)t/15=4×(12)t/5\left(\frac{1}{2}\right)^{t/15} = 4 \times \left(\frac{1}{2}\right)^{t/5}

Rewrite 44 as 222^2:

(12)t/15=(12)t/52\left(\frac{1}{2}\right)^{t/15} = \left(\frac{1}{2}\right)^{t/5 - 2}

Equating the exponents:

t15=t52\frac{t}{15} = \frac{t}{5} - 2 t15t5=2\frac{t}{15} - \frac{t}{5} = -2

Multiply by 1515:

t3t=30t - 3t = -30 2t=30-2t = -30 t=15t = 15

Therefore, the time required for the concentrations to become equal is 15min15 \, \text{min}.

Exponential Form Method

Given: Radioactive decay of both substances starts together. Half-lives are 15min15 \, \text{min} for A and 5min5 \, \text{min} for B. Initially, B has concentration 4x4x if A has concentration xx.

Find: Time at which both concentrations become the same.

Using the exponential decay form:

[A]t=[A]0ekt[A]_t = [A]_0 e^{-kt}

For A:

[A]t=xekAt,kA=ln215[A]_t = x e^{-k_A t}, \qquad k_A = \frac{\ln 2}{15}

So,

[A]t=xe(ln215)t[A]_t = x e^{-\left(\frac{\ln 2}{15}\right)t}

For B:

[B]t=4xekBt,kB=ln25[B]_t = 4x e^{-k_B t}, \qquad k_B = \frac{\ln 2}{5}

So,

[B]t=4xe(ln25)t[B]_t = 4x e^{-\left(\frac{\ln 2}{5}\right)t}

At equal concentrations:

xe(ln215)t=4xe(ln25)tx e^{-\left(\frac{\ln 2}{15}\right)t} = 4x e^{-\left(\frac{\ln 2}{5}\right)t}

Cancel xx:

e(ln215)t=4e(ln25)te^{-\left(\frac{\ln 2}{15}\right)t} = 4 e^{-\left(\frac{\ln 2}{5}\right)t} et(ln25ln215)=4e^{t\left(\frac{\ln 2}{5} - \frac{\ln 2}{15}\right)} = 4

Taking natural logarithm:

t(ln25ln215)=ln4t\left(\frac{\ln 2}{5} - \frac{\ln 2}{15}\right) = \ln 4 tln2(15115)=2ln2t \ln 2 \left(\frac{1}{5} - \frac{1}{15}\right) = 2 \ln 2 t(2ln215)=2ln2t \left(\frac{2\ln 2}{15}\right) = 2 \ln 2 t=15mint = 15 \, \text{min}

Therefore, the correct answer is 1515.

Common mistakes

  • Using the same half-life for both substances is incorrect because A and B decay at different rates. Always write separate decay expressions with t1/2=15mint_{1/2} = 15 \, \text{min} for A and t1/2=5mint_{1/2} = 5 \, \text{min} for B.

  • Ignoring the initial concentration ratio NB=4NAN_B = 4N_A gives a wrong equation. The equality condition must include the factor 44 for substance B before comparing the decayed amounts.

  • Writing 4=(12)24 = \left(\frac{1}{2}\right)^2 is wrong. Since 4=224 = 2^2, in base 12\frac{1}{2} it should be handled carefully as a shift in exponent, leading to the correct exponent equation.

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