Statement Type Chemical Kinetics Questions for NEET
In each of the following questions a statement I is given
followed by a corresponding statement II just below it
of the statements. Mark the correct answer from the following statements.
1. If statement I and statement II are correct and statement II is correct explanation of statement I
2. If statement I and statement II are correct but statement II is not the correct explanation of statement I
3. If statement I is true but statement II is false
4. If statement I is false but statement II is correct
1. Statement I: Rate of reaction decreases with increase in concentration
Statement II: Rate of reaction remains constant for every temperature
2. Statement I: If in a zero-order reaction the con- centration of the reactant is doubled, the half-life period is also doubled
Statement II: For a zero-order reaction, the rate of reaction is independent of initial concentration
3. Statement I: Formation of HI is a bimolecular reaction
Statement II: Two molecules of reactants are involved in this reaction
4. Statement I: If the activation energy of a reaction is zero, temperature will have no effect on the rate constant
Statement II: Lower the activation energy, faster is the reaction
5. Statement I: The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression
Statement II: There are many higher-order reactions
6. Statement I: Hydrolysis of cane sugar is a first- order reaction
Statement II: Water is present in large excess during hydrolysis
7. Statement I: The order of reaction may be negative
Statement II: In some cases, the rate of a reaction decreases with increase in the concentration
8. Statement I: The rate law equation can be found only by experiment
Statement II: It can be written from the stoichiometric equation
9. Statement I: For a zero-order reaction, rate of reaction is independent of conc. of reactants
Statement II: For a zero-order reaction, reaction proceeds at a constant rate which is equal to rate constant of the reaction
10. Statement I: With increase in temperature activa- tion energy of the reaction decreases
Statement II: For every 10° rise in temperature, the rate of the reaction doubles for most of the reactions
11. Statement I: Half-life period is always independent of initial concentration
Statement II: Half-life period is inversely propor- tional to rate constant
12. Statement I: The rate of reaction can also increase with increase in conc. of its product if one of the products acts as catalyst
Statement II: A catalyst lowers the activation energy of reactants
13. Statement I: A catalyst increases the rate of the reaction
Statement II: A catalysed reaction proceeds through a new path having lower activation energy
14. Statement I: For a first-order reaction t1/2 is independent of the initial concentration of reactants
Statement II: For a first-order reaction t1/2 is twice the t3/4.
15. Statement I: In a zero-order reaction, the conc. versus time graph is a straight line
Statement II: The rate change of concentration per unit time in zero-order reaction remains constant
16. Statement I: The order of a reaction is always whole number
Statement II: The molecularity of a reaction is a whole number other than zero, but generally less than 3
17. Statement I: Order of a reaction cannot be written from the balanced equation
Statement II: Rate law can provide some clue about the reaction mechanism
18. Statement I: Molecularity of a reaction cannot be more than three
Statement II: Probability of simultaneous collision between more than three particles is very less
19. Statement I: The reactions having low value of activation energy are generally fast
Statement II: Temperature coefficient for reactions having low activation energy is large
20. Statement I: For any radioactive element the halflife is not dependent on the initial amount of the element taken
Statement II: The radioactive disintegration process is first order reaction
21. Statement I: The enthalpy of reaction remains constant in the presence of a catalyst
Statement II: A catalyst participating in the reaction, forms different activated complex and lowers down the activation energy but the difference in energy of reactant and product remains the same.
22. Statement I: All collisions of reactant molecules lead to product formation
Statement II: Only those collisions in which molecules have correct orientation and sufficient kinetic energy lead to compound formation
23. Statement I: Rate constants determined from Arrhenius equation are fairly accurate for simple as well as complex molecules
Statement II: Reactant molecules undergo chemical change irrespective of their orientation during collision
24. Statement I: First step is always the rate determining step in the path of the reaction
Statement II: Study of kinetics of a reaction can report events only up to the rate-determining step, not beyond that
25. Statement I: At very high concentration of NH3, the decomposition of NH3 on the surface of finely divided catalyst is a zero-order reaction, whereas at lower concentration of NH3 the decomposition becomes a first-order reaction
Statement II: At a lower concentration, the rate of decomposition of NH3 is proportional to the fraction of the catalyst covered
Answer
Class-11
Class-12
1. If statement I and statement II are correct and statement II is correct explanation of statement I
2. If statement I and statement II are correct but statement II is not the correct explanation of statement I
3. If statement I is true but statement II is false
4. If statement I is false but statement II is correct
1. Statement I: Rate of reaction decreases with increase in concentration
Statement II: Rate of reaction remains constant for every temperature
2. Statement I: If in a zero-order reaction the con- centration of the reactant is doubled, the half-life period is also doubled
Statement II: For a zero-order reaction, the rate of reaction is independent of initial concentration
3. Statement I: Formation of HI is a bimolecular reaction
Statement II: Two molecules of reactants are involved in this reaction
4. Statement I: If the activation energy of a reaction is zero, temperature will have no effect on the rate constant
Statement II: Lower the activation energy, faster is the reaction
5. Statement I: The overall order of the reaction is the sum of the exponents of all the reactants in the rate expression
Statement II: There are many higher-order reactions
6. Statement I: Hydrolysis of cane sugar is a first- order reaction
Statement II: Water is present in large excess during hydrolysis
7. Statement I: The order of reaction may be negative
Statement II: In some cases, the rate of a reaction decreases with increase in the concentration
8. Statement I: The rate law equation can be found only by experiment
Statement II: It can be written from the stoichiometric equation
9. Statement I: For a zero-order reaction, rate of reaction is independent of conc. of reactants
Statement II: For a zero-order reaction, reaction proceeds at a constant rate which is equal to rate constant of the reaction
10. Statement I: With increase in temperature activa- tion energy of the reaction decreases
Statement II: For every 10° rise in temperature, the rate of the reaction doubles for most of the reactions
11. Statement I: Half-life period is always independent of initial concentration
Statement II: Half-life period is inversely propor- tional to rate constant
12. Statement I: The rate of reaction can also increase with increase in conc. of its product if one of the products acts as catalyst
Statement II: A catalyst lowers the activation energy of reactants
13. Statement I: A catalyst increases the rate of the reaction
Statement II: A catalysed reaction proceeds through a new path having lower activation energy
14. Statement I: For a first-order reaction t1/2 is independent of the initial concentration of reactants
Statement II: For a first-order reaction t1/2 is twice the t3/4.
15. Statement I: In a zero-order reaction, the conc. versus time graph is a straight line
Statement II: The rate change of concentration per unit time in zero-order reaction remains constant
16. Statement I: The order of a reaction is always whole number
Statement II: The molecularity of a reaction is a whole number other than zero, but generally less than 3
17. Statement I: Order of a reaction cannot be written from the balanced equation
Statement II: Rate law can provide some clue about the reaction mechanism
18. Statement I: Molecularity of a reaction cannot be more than three
Statement II: Probability of simultaneous collision between more than three particles is very less
19. Statement I: The reactions having low value of activation energy are generally fast
Statement II: Temperature coefficient for reactions having low activation energy is large
20. Statement I: For any radioactive element the halflife is not dependent on the initial amount of the element taken
Statement II: The radioactive disintegration process is first order reaction
21. Statement I: The enthalpy of reaction remains constant in the presence of a catalyst
Statement II: A catalyst participating in the reaction, forms different activated complex and lowers down the activation energy but the difference in energy of reactant and product remains the same.
22. Statement I: All collisions of reactant molecules lead to product formation
Statement II: Only those collisions in which molecules have correct orientation and sufficient kinetic energy lead to compound formation
23. Statement I: Rate constants determined from Arrhenius equation are fairly accurate for simple as well as complex molecules
Statement II: Reactant molecules undergo chemical change irrespective of their orientation during collision
24. Statement I: First step is always the rate determining step in the path of the reaction
Statement II: Study of kinetics of a reaction can report events only up to the rate-determining step, not beyond that
25. Statement I: At very high concentration of NH3, the decomposition of NH3 on the surface of finely divided catalyst is a zero-order reaction, whereas at lower concentration of NH3 the decomposition becomes a first-order reaction
Statement II: At a lower concentration, the rate of decomposition of NH3 is proportional to the fraction of the catalyst covered
Answer
| 1 - 4 | 2 - 4 | 3 - 1 | 4 - 2 | 5 - 2 |
| 6 - 1 | 7 - 1 | 8 - 3 | 9 - 2 | 10 - 4 |
| 11 - 4 | 12 - 2 | 13 - 1 | 14 - 3 | 15 - 1 |
| 16 - 4 | 17 - 2 | 18 - 1 | 19 - 3 | 20 - 1 |
| 21 - 1 | 22 - 4 | 23 - 3 | 24 - 4 | 25 - 2 |
Class-11
Class-12
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