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Chapters
2: Solutions
3: Ionic Equilibria
4: Chemical Thermodynamics
5: Electrochemistry
▶ 6: Chemical Kinetics
7: Elements of Groups 16, 17 and 18
8: Transition and Inner transition Elements
9: Coordination Compounds
10: Halogen Derivatives
11: Alcohols, Phenols and Ethers
12: Aldehydes, Ketones and Carboxylic acids
13: Amines
14: Biomolecules
15: Introduction to Polymer Chemistry
16: Green Chemistry and Nanochemistry
![Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 6 - Chemical Kinetics - Shaalaa.com](/images/chemistry-english-12-standard-hsc_6:74400b801d4c44ef8e058ff9d9dfe964.jpg "Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 6 - Chemical Kinetics")
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Solutions for Chapter 6: Chemical Kinetics
Below listed, you can find solutions for Chapter 6 of Maharashtra State Board Balbharati for Chemistry [English] 12 Standard HSC.
Balbharati solutions for Chemistry [English] 12 Standard HSC 6 Chemical Kinetics Exercises [Pages 135 - 137]
Choose the most correct option.
The rate law for the reaction aA + bB → P is rate = k[A] [B]. The rate of reaction doubles if _________.
concentrations of A and B are both doubled.
[A] is doubled and [B] is kept constant
[B] is doubled and [A] is halved
[A] is kept constant and [B] is halved.
Choose the most correct option.
The order of the reaction for which the units of the rate constant are mol dm-3 s-1 is _______.
1
3
0
2
Choose the most correct option.
The rate constant for the reaction \[\ce{2N2O5_{(g)} -> 2N2O4_{(g)} + O2_{(g)}}\] is `4.98 xx 10^-4 "s"^-1`. The order of reaction is _____________.
2
1
0
3
The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be _________.
t
2t
`"t"/2`
3t
Choose the most correct option.
Slope of the graph ln[A]t versus t for first-order reaction is _________.
-k
k
`"k"/2.303`
`"-k"/2.303`
What is the half life of a first order reaction if time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 h?
12 h
3 h
1.5 h
6 h
Choose the most correct option.
The reaction, \[\ce{3ClO- -> ClO^-3 + 2Cl-}\] occurs in two steps,
(i) \[\ce{2ClO- -> ClO^-2}\]
(ii) \[\ce{ClO^-2 + ClO- -> ClO^-_3 + Cl-}\]
The reaction intermediate is _______.
`"Cl"^-`
`"ClO"_2^-`
`"ClO"_3^-`
`"ClO"^-`
Choose the most correct option.
The elementary reaction \[\ce{O3_{(g)} + O_{(g)} -> 2O2_{(g)}}\] is ___________.
unimolecular and second order
bimolecular and first order
bimolecular and second order
unimolecular and first order
Choose the most correct option.
Rate law for the reaction, \[\ce{2NO + Cl2 -> 2NOCl}\] is rate = k[NO2]2[Cl2]. Thus of k would increase with _____________.
increase in temperature
increase of concentration of NO
increase of concentration of Cl2
increase of concentrations of both Cl2 and NO
Choose the most correct option.
For an endothermic reaction, X ⇌ Y. If Ef is the activation energy of the forward reaction and Er that for the reverse reaction, which of the following is correct?
Ef = Er
Ef < Er
Ef > Er
∆H = Ef - Er is negative
Answer the following in one or two sentences.
For the reaction,
\[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\],
what is the relationship among `("d"["N"_2])/"dt"`, `("d"["H"_2])/"dt"` and `("d"["NH"_3])/"dt"`?
Answer the following in one or two sentences.
For the reaction, \[\ce{CH3Br_{(aq)} + OH^{-}_{(aq)} -> CH3OH^{\ominus}_{(aq)} + Br^{\ominus}_{(aq)}}\], rate law is rate = \[\ce{k[CH3Br][OH^\ominus]}\]
How does reaction rate changes if \[\ce{[OH^\ominus]}\] is decreased by a factor of 5?
Answer the following in one or two sentences.
For the reaction,
\[\ce{CH3Br_{(aq)} + OH^-_{ (aq)} -> CH3OH^-_{ (aq)} + Br^-_{ (aq)}}\], rate law is rate = k`["CH"_3"Br"]["OH"^-]`
What is the change in rate if concentrations of both reactants are doubled?
Answer the following in one or two sentences.
What is the relationship between coefficients of reactants in a balanced equation for an overall reaction and exponents in the rate law? In what case the coefficients are the exponents?
Answer the following in one or two sentences.
Why all collisions between reactant molecules do not lead to a chemical reaction?
Answer the following in one or two sentences
What is the activation energy of a reaction?
Answer the following in one or two sentences.
What are the units for rate constants for zero-order and second-order reactions if time is expressed in seconds and concentration of reactants in mol/L?
Answer the following in one or two sentences.
Write the Arrhenius equation and explain the terms involved in it.
Answer the following in one or two sentences.
What is the rate-determining step?
Answer the following in one or two sentences.
Write the relationships between rate constant and half-life of the first order and zeroth-order reactions.
Answer the following in one or two sentences.
How do the half-lives of the first order and zero-order reactions change with the initial concentration of reactants?
Answer the following in brief.
How instantaneous rate of reaction is determined?
Distinguish between Order and Molecularity of reaction.
A reaction takes place in two steps:
- \[\ce{NO_{(g)} + Cl2_{(g)} -> NOCl2_{(g)}}\]
- \[\ce{NOCl2_{(g)} + NO_{(g)} -> 2NOCl_{(g)}}\]
- Write the overall reaction.
- Identify the reaction intermediate.
- What is the molecularity of each step?
Answer the following in brief.
Obtain the relationship between the rate constant and half-life of a first-order reaction.
Answer the following in brief.
How will you represent the zeroth-order reaction graphically?
What are pseudo-first-order reactions?
Answer the following in brief.
Give one example and explain why it is pseudo-first-order.
Answer the following in brief.
What are the requirements for the colliding reactant molecules to lead to products?
Answer the following in brief.
How a catalyst increases the rate of reaction? Explain with the help of a potential energy diagram for catalyzed and uncatalyzed reactions.
Explain with the help of the Arrhenius equation, how do the rate of reaction changes with temperature.
Explain with the help of the Arrhenius equation, how do the rate of reaction changes with activation energy.
Answer the following in brief.
Derive the integrated rate law for the first-order reaction.
How will you represent first order reactions graphically.
Answer the following in brief.
Derive the integrated rate law for the first-order reaction,
\[\ce{A_{(g)} -> B_{(g)} + C_{(g)}}\] in terms of pressure.
Answer the following in brief.
What is a zeroth-order reaction?
Derive the integrated rate law for the zeroth order reaction.
Answer the following in brief.
What are the units of the rate constant?
Answer the following in brief.
How will you determine activation energy graphically using the Arrhenius equation?
Answer the following in brief.
How will you determine activation energy from rate constants at two different temperatures?
Answer the following in brief.
Explain graphically the effect of temperature on the rate of reaction.
Answer the following in brief.
Explain graphically the effect of a catalyst on the rate of reaction.
Answer the following in brief.
For the reaction 2A + B → products, find the rate law from the following data.
| [A]/M | [B]/M | rate/M s-1 |
| 0.3 | 0.05 | 0.15 |
| 0.6 | 0.05 | 0.30 |
| 0.6 | 0.2 | 1.20 |
Solve
In a first-order reaction, the concentration of the reactant decreases from 20 mmol dm-3 to 8 mmol dm-3 in 38 minutes. What is the half-life of reaction?
Solve
The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?
Solve
The energy of activation for a first-order reaction is 104 kJ/mol. The rate constant at 25°C is 3.7 × 10–5 s –1. What is the rate constant at 30°C? (R = 8.314 J/K mol)
Solve
What is the energy of activation of a reaction whose rate constant doubles when the temperature changes from 303 K to 313 K?
The rate constant of a reaction at 500°C is 1.6 × 103 M−1 s−1. What is the frequency factor of the reaction if its activation energy is 56 kJ/mol?
Show that the time required for 99.9% completion of a first-order reaction is three times the time required for 90% completion.
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
The rate constant for the first-order reaction is given by log10 k = 14.34 – 1.25 × 104 T. Calculate activation energy of the reaction.
Solve
What fraction of molecules in a gas at 300 K collide with an energy equal to the activation energy of 50 kJ/mol?
Solutions for 6: Chemical Kinetics
Balbharati solutions for Chemistry [English] 12 Standard HSC chapter 6 - Chemical Kinetics
Shaalaa.com has the Maharashtra State Board Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Balbharati solutions for Mathematics Chemistry [English] 12 Standard HSC Maharashtra State Board 6 (Chemical Kinetics) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry [English] 12 Standard HSC chapter 6 Chemical Kinetics are Pseudo First Order Reaction, First Order Reactions, Chemical Kinetics, Rate of Reactions, Rate of Reaction and Reactant Concentration, Molecularity of Elementary Reactions, Collision Theory of Bimolecular Reactions, Temperature Dependence of Reaction Rates, Effect of a Catalyst on the Rate of Reaction, Integrated Rate Law for Gas Phase f Reactions, Zero Order Reactions, Half Life Period of a Reaction, Integrated Rate Equations.
Using Balbharati Chemistry [English] 12 Standard HSC solutions Chemical Kinetics exercise by students is an easy way to prepare for the exams, as they involve solutions arranged chapter-wise and also page-wise. The questions involved in Balbharati Solutions are essential questions that can be asked in the final exam. Maximum Maharashtra State Board Chemistry [English] 12 Standard HSC students prefer Balbharati Textbook Solutions to score more in exams.
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