1st Year Chemistry Reaction Kinetics MCQs

On this page, we are going to share 1st Year Chemistry Reaction Kinetics MCQs with the students. You can prepare for the entry test accordingly. In Reaction Kinetics, the characteristics of Chemical reactions and the factors affecting them are studied. Every reaction has its rate, which defines its progress speed concerning time. In chemical reactions, the Half-Period took great importance. The rate of Chemical reaction is determined by a unique formula. Some physical and chemical methods are also used for this purpose. Activation energy plays an important part in reactions. Many factors affect the rate of reactions. Catalysts play a unique role in chemical reactions. They make the reaction quite efficient. So, this is a brief introduction to this chapter. Check the important MCQs with their answers given below.

1st Year Chemistry Reaction Kinetics MCQs

KEY POINTS

Question#1. The activation energy of reaction:

• Includes the average kinetic energy of the reactants
• Is in addition to the average kinetic energy of the reactants
• Is in addition to the average kinetic energy of the products
• Required for effective collisions

Question#2. E_a appears as a potential energy hill between _________ for carrying out the reaction:

• Among the reactants
• Reactants and the products
• Among the products
• None of the above

Question#3. The slope of the curve between 1/T and log k gives:

• Reaction rate
• Both of the above
• Specific rate constant
• Activation energy

Question#4. The unit of the rate constant is the same as that of the rate of reaction in:

• 1^st order reaction
• Zero-order reaction
• 2^nd order reaction
• 3^rd order reaction

Question#5. Arrhenius equation can be used for evaluating:

• Specific rate constant
• Both of the above
• Activation energy
• Half-life period

Question#6. A catalyst can:

• Accelerate the reaction rate
• Retard the reaction rate
• Chemically un-consumed at the end of the reaction
• All of the above

Question#7. The 2^nd order reaction becomes 1^st when:

• One of the reactants is limiting
• One of the reactants is in large excess
• None of the reactants is in large excess
• One of the reactants is acidic

Question#8. Oxidation of SO_2(g) in the presence of NO_(g) catalyst is an example of:

• Homogeneous catalysis
• Autocatalysis
• Heterogeneous catalysis
• Negative catalysis

Question#9. Oxidation of SO_2(g) in the presence of V₂O_5(s) is an example of:

• Homogeneous catalysis
• Autocatalysis
• Heterogeneous catalysis
• Negative catalysis

Question#10. Which one of the following is not a characteristic of a catalyst:

• It is specific in its action
• Provides the reactants a low activation energy barrier
• Becomes chemically changed at the end of a reaction
• It can be poisoned by an impurity which deactivates its catalytic capability

Question#11. The specific rate constant of a chemical reaction is the rate of the reaction when the concentration of the reactant is:

• Less than unity
• Greater than unity
• Equal to unity
• Equal to the concentration of 2^nd order reaction

Question#12. The half life for a 1^st order decomposition of a substance dissolved in CCl₄ is 2.5 hours at 30°C. The amount of substance left after 10 hours if the initial weight of the substance is 160g:

• 5g
• 15g
• 10
  
• 20g

Question#13. An endothermic reaction A → B has an activation energy 15kcal /mol and the heat of reaction 5kcal/mol. The activation energy for the reaction B → A will be:

• 20kcal/mol
• 10kcal/mol
• 15kcal/mol
• None of the above

Question#14. The rate of reaction is doubled for every 10°C rise in temperature. The increase in reaction rate as a result of temperature rise from 10°C to 100°C is:

• 112
• 400
• 512
  
• 614

Question#15. For the 1^st order decomposition reaction 2N₂O₅ (g) → 4NO_2(g) + O_2(g) the half-life is given as:

• 0.693/k
• log2/k
• 0.693/2k
• ln2/k

Question#16. Which one of the following is correct about the following reaction if the iron is not 100% pure?
                     2Fe + 3H₂O + O₂ → Fe₂O₃.3H₂O

• Very fast reaction
• Moderately reaction
• Very slow reaction
• Not predicted

Question#17. For a chemical reaction to occur:

• The vessel shall be open
• Reacting molecules should have less energy than Ea at the time of the collision
• Reacting molecules must be properly oriented and energy more than or equal to Ea
• The reacting molecules must not collide with each other

Question#18. The reaction that involves gases, its rate does not depend upon?

• Catalyst
• Partial pressure
• Temperature
• Moles dm^-3

Question#19. The mathematical relation between the rate of reaction and the concentrations of the reactants is known as the:

• Rate equation
• Arrhenius equation
• Rate low
• Both a and c

Question#20. Which one affects the specific rate constant?

• Temperature
• Concentration of reactants
• Catalyst
• All of these

Question#21. Which one is a chemical method for the determination of the rate of reaction?

• Spectrometry
• Refractrometric method
• Dilatometric method
• Titration

Question#22. When the concentration of a reactant in the reaction is increased by 8 times, the rate increased only by 2 times. The order of the reaction is:

• 1
• ½
• 1/3
• 2

Question#23. The rate expression for a reaction A+B → products is rate = k [A]^2/3 [B]^-1/2 the order of reaction is:

• 0
• 5/2
• 3/2
• 1

Question#24. If 75% of any given amount of radioactive element disintegrates in 60 min. The half life of a radioactive element is.

• 20 min
• 30 min
• 45 min
• 25 min

Question#25. The unit of rate constant depends on?

• Number of reactants
• Order of reaction
• Concentration terms
• Molecularity of reaction

Question#26. The unit of the rate constant of a second-order reaction is:

• mol dm^-3 sec^-1
• mol^-2 dm⁺⁶
• sec^-1
• mol^-1 dm⁺³ sec^-1

Question#27. The half-life period of the zero-order reaction is equal to:

• 0.693/K
• 1/Ka
• a/2
• 1.5/Ka²

Question#28. The influence of temperature on the reaction rate is predicted by:

• Free energy change of reaction
• Arrhenius equation
• Van der Waal’ equation
• Kinetic equation

Question#29. If the energy of the activated complex lies close to the energy of reactants, it means that reaction is:

• Slow
• Endothermic
• Exothermic
• Exothermic and fast

Question#30. Which of the following statements regarding a catalyst is not true?

• A catalyst does not alter the equilibrium in a reversible reaction
• A catalyst can initiate the reaction which is not thermodynamically favorable
• Catalytic reactions are very specific
• A catalyst remains unchanged in composition and quantity