- Keneitsino Lydia
- March 5, 2026
30 Integrated Equation Solved MCQs Chemistry: Problems to Master Concepts for NEET, JEE & CUET
Integrated Equation Solved MCQs Chemistry is a highly important preparation topic for aspirants studying chemical kinetics in Class 12 and preparing for competitive examinations. A strong grasp of Integrated Equation Solved MCQs Chemistry helps aspirants connect rate laws with time-dependent concentration changes. Without understanding Integrated Equation Solved MCQs Chemistry , it becomes difficult to solve numerical problems related to half-life, percentage completion, and rate constant calculations.
In chemical kinetics, integrated rate equations are derived by integrating differential rate laws. The purpose of Integrated Equation Solved MCQs Chemistry is to test whether aspirants can apply these equations in real numerical contexts. For zero order reactions, the integrated equation is:
[A] = [A]₀ − kt
When practicing Integrated Equation Solved MCQs Chemistry , aspirants must recognize that a straight-line plot of concentration versus time indicates zero order behavior. The slope of this graph equals −k. Many Integrated Equation Solved MCQs Chemistry revolve around interpreting graphical data to determine reaction order and rate constant.
For first order reactions, the integrated equation is:
ln[A] = ln[A]₀ − kt
or
k = (2.303/t) log([A]₀/[A])
Understanding these forms is essential while solving Integrated Equation Solved MCQs Chemistry because exam questions often present data in logarithmic form. Aspirants should be comfortable converting between natural logarithm and base-10 logarithm when handling Integrated Equation Solved MCQs Chemistry . Careful substitution and correct unit handling prevent calculation errors.
Second order reactions follow a different integrated form:
1/[A] = 1/[A]₀ + kt
In Integrated Equation Solved MCQs Chemistry , this equation is frequently used to determine whether a reaction follows second order kinetics. A linear plot of 1/[A] versus time confirms second order behavior. Recognizing such graphical patterns is a key strategy in Integrated Equation Solved MCQs Chemistry .
Another important area covered under Integrated Equation Solved MCQs Chemistry is percentage completion. For example, if a problem states that 75% of a reaction is completed, aspirants must understand that only 25% of the initial concentration remains. Many Integrated Equation Solved MCQs Chemistry require combining the concept of fractional conversion with the appropriate integrated equation. This layered approach tests conceptual clarity rather than memorization.
Temperature dependence is also indirectly tested through Integrated Equation Solved MCQs Chemistry . Although the Arrhenius equation determines how k changes with temperature, once k is known, the integrated equation helps determine concentration at any given time. Aspirants preparing through Integrated Equation Solved MCQs Chemistry learn to bridge kinetic theory with numerical execution.
Graphical interpretation is a major component of Integrated Equation Solved MCQs Chemistry . For instance, if ln[A] versus time gives a straight line, the reaction is first order. If [A] versus time is linear, it is zero order. If 1/[A] versus time is linear, it is second order. Many Integrated Equation Solved MCQs Chemistry test the ability to quickly identify the correct integrated form from graph shape alone.
Accuracy in solving Integrated Equation Solved MCQs Chemistry depends on systematic steps. First, identify the order of reaction. Second, write the correct integrated equation. Third, substitute values carefully. Finally, ensure unit consistency. Repeated practice of Integrated Equation Solved MCQs Chemistry improves speed and reduces calculation anxiety in examinations.
Another frequently tested concept in Integrated Equation Solved MCQs Chemistry is half-life derivation from integrated equations. For first order reactions, t₁/₂ = 0.693/k, which is derived from the first order integrated equation. Many Integrated Equation Solved MCQs Chemistry combine half-life with concentration-time relationships to test deeper understanding.
Integrated Equation Solved MCQs Chemistry:
1. Slope of First Order Plot
Q1. For first order reaction, the value of slope for graph of
log([R]₀/[R]) vs t is:
A. k2.303\frac{k}{2.303}
B. 2.303k\frac{2.303}{k}
C. −k
D. −k2.303-\frac{k}{2.303}
Answer: A
2. Assertion–Reason (Zero Order)
Q2.
Assertion: If in a zero order reaction, concentration is doubled, half-life doubles.
Reason: For zero order reaction, rate is independent of initial concentration.
A. Both correct and Reason explains Assertion
B. Both correct but Reason does not explain Assertion
C. Assertion correct, Reason incorrect
D. Both incorrect
Answer: B
3. Order from Experimental Data
Q3. Decomposition of ammonium nitrite data suggests order:
A. Zero
B. One
C. Two
D. Three
Answer: B
4. First Order Time Comparison
Q4. For first order reaction, time for second condition is:
A. 1 h
B. 0.5 h
C. 0.25 h
D. 2 h
Answer: A
5. Molecularity of Slow Step
Q5. Total order = 2 and step-2 is slow. Molecularity of step-2:
A. 1
B. 2
C. 3
D. 4
Answer: B
6. Pseudo First Order Reaction
Q6. Rate constant of pseudo first order reaction:
A. Depends on reactant in small amount
B. Depends on reactant in excess
C. Independent of concentration
D. Depends only on temperature
Answer: A
7. Fractional Order Reaction
Q7. Order of reaction: rate = k[A]³ᐟ²[B]⁻¹
A. 3/2
B. 1/2
C. 1/4
D. 4
Answer: B
8. Mechanism Based Order
Q8. Order of overall reaction:
A. 2
B. 2
C. 1
D. Zero
Answer: B
9. Higher Order Reactions Rare
Q9. Reason higher order reactions are rare:
A. Shifting equilibrium
B. Loss of active species
C. Low probability of simultaneous collision
D. Increase in entropy
Answer: C
10. Time for 99% Completion
Q10. For first order reaction, time for 99% completion:
A. 4.606k\frac{4.606}{k}
B. 2.303k\frac{2.303}{k}
C. 0.693k\frac{0.693}{k}
D. 6.909k\frac{6.909}{k}
Answer: A
11. Two-Third Life
Q11. Two-third life for first order reaction:
A. 2.005 × 10¹³ sec
B. 2.005 × 10¹⁴ sec
C. 5.002 × 10¹³ sec
D. 5.002 × 10¹⁴ sec
Answer: A
12. First Order Reaction
Q12. In a first order reaction, the rate of reaction mainly depends on:
A. Concentration of one reactant
B.Temperature
C.Pressure only
D. Catalyst only
Answer: A
13. Time Ratio (75% / 50%)
Q13. Ratio:
A. 2
B. 1
C. 3
D. 4
Answer: A
14. Arrhenius Based Calculation
Q14. Value of x:
A. 2
B. 4
C. 8
D. 16
Answer: D
15. Rate Constant from Data
Q15. Rate constant:
A. 5
B. 1.2
C. 2
D. 50
Answer: D
16. Overall Order
Q16. Rate = k[A]¹ᐟ²[B]³ᐟ²
A. Second order
B. First order
C. Zero order
D. Third order
Answer: A
17. Isomerization Time
Q17. Time required:
A. 26
B. 30
C. 36
D. 20
Answer: A
18. First Order Concentration Variation
Q18.
A. 1/C increases linearly
B. log C decreases linearly
C. C decreases with 1/t
D. log C decreases with 1/t
Answer: B
19. Incorrect Statement
Q19.
A. Unit of rate disappearance is M s⁻¹
B. Unit of rate reaction is M s⁻¹
C. Unit of k depends on order
D. Unit of k for first order is M s⁻¹
Answer: D
20. Zero Order Half-Life Plot
Q20.
A. Straight line slope = k
B. Horizontal line
C. Straight line slope = −k
D. Straight line slope = 1/(2k)
Answer: D
21. First Order Time Calculation
Q21.
A. 1.30 h
B. 21.60 h
C. 0.36 h
D. 2.60 h
Answer: C
22. First Order (1/16th)
Q22.
A. 2.3 × 10⁻²
B. 9.5 × 10⁻²
C. 4.6 × 10⁻²
D. 6.9 × 10⁻²
Answer: C
23. Molecularity & Order
Q23.
A. 1 and 1
B. 2 and 3/2
C. 2 and 1
D. 3/2 and 2/3
Answer: B
24. Integrated equation of a reaction
Q24. The integrated equation of a reaction is mainly used to determine:
A. Colour of the reaction
B. Rate Constant
C. Temperature
D. Pressure
Answer: B
25. True Statement
Q25.
A. Second order always multistep
B. Zero order always multistep
C. First order always single step
D. Zero order single step
Answer: B
26. 75% and 60% Completion
Q26.
A. 40
B. 50
C. 60
D. 30
Answer: C
27. Equal Initial Concentration Problem
Q27.
A. 180
B. 240
C. 300
D. 900
Answer: D
28. Order Sequence from Graph
Q28.
A. D > A > B > C
B. A > B > C > D
C. B > A > C > D
D. C > A > B > D
Answer: A
29. 60% and 93.6% Completion
Q29.
A. 100 min
B. 83.8 min
C. 50 min
D. 150 min
Answer: D
30. Graph with Zero Intercept
Q30.
A. log [R] vs t
B. log([R]₀/[R]) vs t
C. log K vs 1/T
D. [R] vs t
Answer: B
Conclusion on Integrated Equation Solved MCQs Chemistry
In conclusion, Integrated Equation Solved MCQs Chemistry form a foundational pillar of chemical kinetics preparation. Mastery of Integrated Equation Solved MCQs Chemistry enables aspirants to confidently handle zero, first, and second order numerical problems. Consistent practice of Integrated Equation Solved MCQs Chemistry builds conceptual clarity, improves calculation speed, and ensures higher scoring potential in board and competitive examinations.