Chemical Kinetics involve the study of rates of chemical reactions. This also includes the reaction pathways and the mechanism of the reaction. The factors that affect the rate of a reaction, the effect of change of concentration on the rate of the reaction and the order of the reaction are also studied well in this chapter.
Download Class 12 Chemistry Worksheet on Chapter 4 Chemical Kinetics Set 1 PDF
CBSE Class 12 Chemistry Chapter 4 Chemical Kinetics Worksheet – Set 1
Q-1: Which statement is not true about the order of a reaction?
a.) Order is independent of the stoichiometric coefficients of the reactants.
b.) The order of a reaction cannot be fractional.
c.) Order is the sum of the powers of the concentration of reactants present in the rate law expression.
d.) Order can be determined experimentally.
Q-2: The applicability of collision theory is on
a.) Intramolecular reactions
b.) Bimolecular reactions
c.) Zero order reactions
d.) First order reaction
Q-3: Find the order of a reaction that gets 50% completed in 2 hours and 75% completed in 4 hours.
Q-4: The range of temperature coefficient for the most of the reactions is:
a.) 1 to 3
b.) 2 to 3
c.) 1 to 4
d.) 2 to 4
Q-5: List 4 factors that affect the rate of a chemical reaction.
Q-6: The rate of a reaction becomes double when the temperature is increased by 10 K because
a.) Ea decreases as the temperature increases
b.) The higher temperature is proportional to the number of colliding particles that cross the energy barrier.
c.) The collisions occur with more energy
d.) The strength of the bonds of the reactants decreases as the temperature increases
Q-7: Write the rate law expression for the reaction:
2NO (g) + O2 (g) → 2NO2 (g)
Q-8: Differentiate between a first order and a second order reaction.
Q-9: The minimum value of activation energy (Ea) for an endothermic reaction is
a.) less than ΔH
b.) more than ΔH
c.) equal to ΔH
d.) zero
Q-10: Sucrose decomposes into glucose and fructose in an acidic medium and obeys the first order rate law. Calculate the fraction of sucrose left after 8 hours if the half life period for sucrose is 3 hours.
Q-11: Hydrogen peroxide is decomposed in an alkaline medium catalysed by the iodide ions.
The reaction for the same proceeds in two steps as:
Step-1: H2O2 + I– → H2O + IO– (slow)
Step-2: H2O2 + IO– → H2O + I– + O2 (fast)
(a.) Write the expression for the rate law.
(b.) Determine the order of the reaction with respect to hydrogen peroxide.
Q-12: What is the molecularity of a reaction?
Q-13: Why do catalysts not have any effect on the equilibrium constant of a reaction?
Q-14: Consider the following reaction:
C12H22O11 + H2O 
C6H12O6 + C6H12O6
(a.) Write the expression for the rate of the reaction.
(b.) Write the rate law expression.
(c.) Determine the molecularity of the reaction.
(d.) Determine the order of the reaction.
Q-15: The unit of rate constant for a reaction is L mol-1 s-1. The order of the reaction is ___.
a.) 0
b.) 1
c.) 2
d.) 3
Q-16: Illustrate the effect of using a catalyst on the activation energy of the reaction graphically.
Q-17: Which of the following does not truly express the reaction rate for the following reaction?
2A + B → 3C + D
a.) d[D]/dt
b.) -d[C]/3dt
c.) -d[A]/2dt
d.) -b[B]/dt
Q-18: For the reaction A → Products, the value of k is 4.5 x 103 s-1 and that of the activation energy is 60 kJ mol-1 at 10 oC. Determine the temperature at which the value of k will be 1.5 x 104 s-1.
Q-19: What is the molecularity and the order of the following reaction?
A + H2O → B, Rate = k[A]
Q-20: Under what condition can a bimolecular reaction convert into a reaction kinetically of first order?
Download the PDF to access answers to the Chemistry Worksheet for Class 12 Chemistry Chapter 4 Chemical Kinetics Set -1.
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