Pre-exponential factors of two different reactions of same order are identical. Let activation energy of first reaction exceeds the activation energy of second reaction by 20text kJ mol^-1$20\text{ kJ mol}^{-1}$. If k_1$k_{1}$ and k_2$k_{2}$ are the rate constants of first and second reaction respectively at 300 K, then ln frack_2k_1$\ln \frac{k_{2}}{k_{1}}$ will be ..... (nearest integer) [R=8.3text J K^-1text mol^-1]$[R=8.3\text{ J K}^{-1}\text{ mol}^{-1}]$
Numerical Answer Type:
Enter a numerical valueAnswer: 8 to 8+4 marks
Solution & Explanation
### Related Formula
ln k = ln A - fracE_aRT$$\ln k = \ln A - \frac{E_a}{RT}$$
### Core Logic
For Reaction 1: ln k_1 = ln A - fracE_1RT$\ln k_1 = \ln A - \frac{E_1}{RT}$
For Reaction 2: ln k_2 = ln A - fracE_2RT$\ln k_2 = \ln A - \frac{E_2}{RT}$
(Pre-exponential factor A$A$ is the same).
Subtracting the first from the second:
ln k_2 - ln k_1 = -fracE_2RT - left(-fracE_1RTright)$$\ln k_2 - \ln k_1 = -\frac{E_2}{RT} - \left(-\frac{E_1}{RT}\right)$$ln left(frack_2k_1right) = fracE_1 - E_2RT$$\ln \left(\frac{k_2}{k_1}\right) = \frac{E_1 - E_2}{RT}$$
Given that E_1$E_1$ exceeds E_2$E_2$ by 20text kJ mol^-1$20\text{ kJ mol}^{-1}$, E_1 - E_2 = 20000text J mol^-1$E_1 - E_2 = 20000\text{ J mol}^{-1}$.
T = 300text K$T = 300\text{ K}$, R = 8.3text J K^-1text mol^-1$R = 8.3\text{ J K}^{-1}\text{ mol}^{-1}$.
ln left(frack_2k_1right) = frac200008.3 times 300 = frac2008.3 times 3 = frac20024.9$$\ln \left(\frac{k_2}{k_1}\right) = \frac{20000}{8.3 \times 300} = \frac{200}{8.3 \times 3} = \frac{200}{24.9}$$ln left(frack_2k_1right) = 8.032$$\ln \left(\frac{k_2}{k_1}\right) = 8.032$$
Rounding off to nearest integer gives 8.
### Evaluation Rubric / Model Answer
null
### Chapter Mix
Class 12 Chemistry: Chemical Kinetics
Keywords:#Arrhenius equation ratio#ln(k2/k1)#JEE Main 2026 Morning Q71#Chemical Kinetics JEE Main 2026
More Chemical Kinetics Previous-Year Questions — Page 5
Q40jee_main_2025_28_jan_eveningFirst Order Kinetics
For bacterial growth in a cell culture, growth law is very similar to the law of radioactive decay. Which of the following graphs is most suitable to represent bacterial colony growth?
A. (1)
B. (2)
C. (3)
D. (4)
Solution
### Related Formula
Exponential growth equation model:
N = N_0 e^Kt$N = N_0 e^{Kt}$
Normalized configuration formula:
fracNN_0 = e^Kt$$\frac{N}{N_0} = e^{Kt}$$
### Core Logic
Radioactive decay follows a decreasing exponential path (N = N_0 e^-lambda t$N = N_0 e^{-\lambda t}$).
Conversely, cell culture growth functions via an *increasing* exponential pattern because the rate of growth is directly proportional to the current population size (dN/dt = KN$dN/dt = KN$). This results in an exponential curve that starts at fracNN_0 = 1$\frac{N}{N_0} = 1$ when t = 0$t = 0$ and curves sharply upward over time.
### Step 1: Finding the Matching Curve
Plotting fracNN_0$\frac{N}{N_0}$ against time shows an upward-clinging exponential profile starting from 1$1$, which perfectly matches the curve in option (4).
Exponential growth profile plot for Q40
### Pattern Recognition
The expression e^Kt$e^{Kt}$ dictates an exponential increase. Ensure the curve starts from a non-zero value (1$1$) at t=0$t=0$, as fracN_0N_0 = 1$\frac{N_0}{N_0} = 1$, rather than starting from the origin (0$0$).
### Evaluation Rubric / Model Answer
null
### Chapter Mix
Class 12 Chemistry: Chemical Kinetics
Qjee_main_2025_29_jan_morningReaction Mechanism and Rate Law
The reaction mathrmA_2 + mathrmB_2
ightarrow 2$\mathrm{A}_2 + \mathrm{B}_2
ightarrow 2$ AB follows the mechanism
mathrm A _ 2 xrightarrow [ mathrm k _ - 1 ]mathrm k _ 1 mathrm A + mathrm A text (fast) $$\mathrm {A} _ {2} \xrightarrow [ \mathrm {k} _ {- 1} ]{\mathrm {k} _ {1}} \mathrm {A} + \mathrm {A} \text{ (fast)} $$mathrm A + mathrm B _ 2 xrightarrow mathrm k _ 2 mathrm A B + mathrm B text (slow)$$\mathrm {A} + \mathrm {B} _ {2} \xrightarrow {\mathrm {k} _ {2}} \mathrm {A B} + \mathrm {B} \text{ (slow)}$$mathrm A + mathrm B
ightarrow mathrm A B text (fast)$$\mathrm {A} + \mathrm {B}
ightarrow \mathrm {A B} \text{ (fast)}$$
The overall order of the reaction is :
A. 1.5
B. 3
C. 2.5
D. 2
Solution
### Related Formula
textRate = k cdot [textReactants]^textorder$$\text{Rate} = k \cdot [\text{Reactants}]^{\text{order}}$$
### Core Logic
The slowest elementary step controls the net kinetic pathway rate law :
textRate = k_2[mathrmA][mathrmB2] quad dots textEquation (1)$$\text{Rate} = k_2[\mathrm{A}][\mathrm{B}2] \quad \dots \text{Equation (1)}$$
Since [mathrmA]$[\mathrm{A}]$ behaves as a transient intermediate species, replace it using the prior fast equilibrium step :
frack_1k-1 = frac[mathrmA]^2[mathrmA2] implies [mathrmA]^2 = left(frack_1k-1right) [mathrmA2]$$\frac{k_1}{k{-1}} = \frac{[\mathrm{A}]^2}{[\mathrm{A}2]} \implies [\mathrm{A}]^2 = \left(\frac{k_1}{k{-1}}\right) [\mathrm{A}2]$$[mathrmA] = sqrtfrack_1k-1 cdot [mathrmA2]^1/2$$[\mathrm{A}] = \sqrt{\frac{k_1}{k{-1}}} \cdot [\mathrm{A}2]^{1/2}$$
Substitute [mathrmA]$[\mathrm{A}]$ back into Equation (1) :
textRate = k_2 sqrtfrack_1k-1 cdot [mathrmA2]^1/2[mathrmB2]$$\text{Rate} = k_2 \sqrt{\frac{k_1}{k{-1}}} \cdot [\mathrm{A}2]^{1/2}[\mathrm{B}2]$$
Sum of powers determining overall order:
textOrder = frac12 + 1 = 1.5$$\text{Order} = \frac{1}{2} + 1 = 1.5$$
Hence, Option (1) is correct.
### Pattern Recognition
Whenever a fast initial step dissociates a molecule into matching independent halves, it always injects a fractional order component of 0.5$0.5$ relative to that parent species.
Q84jee_main_2024_01_february_morningKinetics of Radioactive Decay
The ratio of frac^14mathrmC^12mathrmC$\frac{^{14}\mathrm{C}}{^{12}\mathrm{C}}$ in a piece of wood is frac18$\frac{1}{8}$ part that of atmosphere. If half life of ^14mathrmC$^{14}\mathrm{C}$ is 5730 years, the age of wood sample is .... years.
Numerical Answer.Answer: 17190 to 17190
Solution
### Related Formula
N = fracN_02^n$$N = \frac{N_0}{2^n}$$
where n = fractt_1/2$n = \frac{t}{t_{1/2}}$ (number of half-lives).
Alternatively, using the first-order decay formula:
t = frac2.303lambda log left( fracN_0N_t right)$$t = \frac{2.303}{\lambda} \log \left( \frac{N_0}{N_t} \right)$$
where lambda = frac0.693t_1/2$\lambda = \frac{0.693}{t_{1/2}}$.
### Core Logic
The atmospheric ratio of ^14mathrmC/^12mathrmC$^{14}\mathrm{C}/^{12}\mathrm{C}$ acts as the initial activity or amount (N_0$N_0$) when the tree was alive.
The current ratio in the wood represents the amount left at time t$t$ (N_t$N_t$).
Given that N_t = frac18 N_0$N_t = \frac{1}{8} N_0$.
### Step 1: Calculate Half-lives
fracN_tN_0 = frac18$$\frac{N_t}{N_0} = \frac{1}{8}$$ left(frac12right)^n = frac18 = left(frac12right)^3$$ \left(\frac{1}{2}\right)^n = \frac{1}{8} = \left(\frac{1}{2}\right)^3$$
So, the number of half-lives passed, n = 3$n = 3$.
### Step 2: Calculate Age
t = n times t_1/2$$t = n \times t_{1/2}$$t = 3 times 5730 text years$$t = 3 \times 5730 \text{ years}$$t = 17190 text years$$t = 17190 \text{ years}$$
### Pattern Recognition
Whenever the remaining fraction is a perfect power of 1/2$1/2$ (like 1/2, 1/4, 1/8, 1/16$1/2, 1/4, 1/8, 1/16$), just find the exponent n$n$ and multiply by t_1/2$t_{1/2}$. Here, 1/8 = (1/2)^3 rightarrow 3$1/8 = (1/2)^3 \rightarrow 3$ half-lives.
### Evaluation Rubric / Model Answer
null
### Chapter Mix
Class 12 Chemistry: Chemical Kinetics
Q87jee_main_2024_29_january_eveningFirst Order Kinetics and Half Life
The half-life of radioisotopic bromine - 82 is 36 hours. The fraction which remains after one day is ________ times 10^-2$\times 10^{-2}$. (Given antilog 0.2006 = 1.587)
Numerical Answer.Answer: 63 to 63
Solution
### Related Formula
k = frac0.693,
t_1/2 quad textand quad t = frac2.303,
k log_10 left(fraca,
a-xright)$$k = \frac{0.693},
{t_{1/2}} \quad \text{and} \quad t = \frac{2.303},
{k} \log_{10} \left(\frac{a},
{a-x}\right)$$
### Core Logic
Given t_1/2 = 36text hours$t_{1/2} = 36\text{ hours}$, calculate the decay constant (k$k$):
k = frac0.693,
36 = 0.01925text hr^-1$$k = \frac{0.693},
{36} = 0.01925\text{ hr}^{-1}$$
We want to find the fraction remaining after 1text day = 24text hours$1\text{ day} = 24\text{ hours}$:
log_10 left(fraca,
a-xright) = frack times t,
2.303 = frac0.01925 times 24,
2.303 = 0.2006$$\log_{10} \left(\frac{a},
{a-x}\right) = \frac{k \times t},
{2.303} = \frac{0.01925 \times 24},
{2.303} = 0.2006$$
### Step 1: Antilog Application
Taking the antilog on both sides:
fraca,
a-x = 1.587 implies textFraction remaining left(fraca-x,
aright) = frac1,
1.587 approx 0.6301$$\frac{a},
{a-x} = 1.587 \implies \text{Fraction remaining } \left(\frac{a-x},
{a}\right) = \frac{1},
{1.587} \approx 0.6301$$
Expressing the remaining fraction in the requested format:
0.6301 = 63 times 10^-2$$0.6301 = 63 \times 10^{-2}$$
Thus, the required integer value is **63**.
### Pattern Recognition
Ensure all time variables are in matching units (hours) before substituting values into first-order kinetic equations.
### Evaluation Rubric / Model Answer
null
### Chapter Mix
Class 12 Chemistry: Chemical Kinetics
Q82jee_main_2024_27_jan_morningDetermination of Order of Reaction
Consider the following data for the given reaction:
2textHI_(g) rightarrow textH_2(g) + textI_2(g)$$2\text{HI}_{(g)} \rightarrow \text{H}_{2(g)} + \text{I}_{2(g)}$$
Experiment
[textHI] text (mol L^-1text)$[\text{HI}] \text{ (mol L}^{-1}\text{)}$
The order of the reaction is textquadquad$\text{\quad\quad}$.
Numerical Answer.Answer: 2 to 2
Solution
### Related Formula
Rate law relation expression:
R = k[textHI]^n$$R = k[\text{HI}]^n$$
where n$n$ represents the overall reaction order indicator.
### Step 1: Set up ratios using data subsets
Comparing data from experiment 1 and experiment 2:
fracR_2R_1 = frac3.0 times 10^-37.5 times 10^-4 = left(frac0.010.005right)^n$$\frac{R_2}{R_1} = \frac{3.0 \times 10^{-3}}{7.5 \times 10^{-4}} = \left(\frac{0.01}{0.005}\right)^n$$4 = (2)^n$4 = (2)^n$2^2 = 2^n implies n = 2$$2^2 = 2^n \implies n = 2$$
### Pattern Recognition
Doubling concentration (0.005 rightarrow 0.01$0.005 \rightarrow 0.01$) increases the reaction rate by 4 times (7.5 times 10^-4 rightarrow 3.0 times 10^-3$7.5 \times 10^{-4} \rightarrow 3.0 \times 10^{-3}$). Hence, it is a clear second-order (2^2 = 4$2^2 = 4$) dynamic pattern.
### Chapter Mix
Class 12 Chemistry: Chemical Kinetics
More Chemical Kinetics Questions — jee_main_2026_21_jan_morning
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