CBSE Class 12 Chemistry Chemical Kinetics Worksheet Set E

Read and download free pdf of CBSE Class 12 Chemistry Chemical Kinetics Worksheet Set E. Students and teachers of Class 12 Chemistry can get free printable Worksheets for Class 12 Chemistry in PDF format prepared as per the latest syllabus and examination pattern in your schools. Standard 12 students should practice questions and answers given here for Chemistry in Grade 12 which will help them to improve your knowledge of all important chapters and its topics. Students should also download free pdf of Class 12 Chemistry Worksheets prepared by school teachers as per the latest NCERT, CBSE, KVS books and syllabus issued this academic year and solve important problems provided here with solutions on daily basis to get more score in school exams and tests

Chemical Kinetics Class 12 Chemistry Worksheet Pdf

Class 12 Chemistry students should refer to the following printable worksheet in Pdf for Chemical Kinetics in standard 12. This test paper with questions and answers for Grade 12 Chemistry will be very useful for exams and help you to score good marks

Class 12 Chemistry Worksheet for Chemical Kinetics

CHEMICAL KINETICS

Q1) Define

a) rate of a reaction

b) activation energy

Q2) The decomposition of PH3 follows the following reaction

4PH3 →P4 + 6H2

Rate equation is → Rate = k [PH3]. The Half life of PH3 is 37.9 sec at 120°C

a) How much time is required for 3/4th of PH3 to decompose? Ans[75.82 sec]

b) What fraction of the original sample of PH3 remains behind after one minute? Ans[2.995]

Q3) Define

a) order of reaction

b) molecularity of a reaction

Q4) the rate of a reaction increases four times when the temperature changes from 300K to 320K. Find the activation energy. (R=8.314 J/K/mol) Ans [35.34 KJ/mol]

Q5) A reaction is of first order in reactant A and of second order in reactant B. How is the rate of this reaction affected when a) conc. Of B alone is increased to 3 times? b) the conc. A as well as B are doubled? 


Important Questions for NCERT Class 12 Chemistry Chemical Kinetics

 

Question. For reaction aA→ xP , when [A] = 2.2 mM, the rate was found to be 2.4 mMs–1. On reducing concentration of A to half, the rate changes to 0.6 mMs–1. The order of reaction with respect to A is : 
(a) 1.5
(b) 2.0
(c) 2.5
(d) 3.0

Answer   B

Question. For a first order reaction, to obtain a positive slope, we need to plot {where [A] is the concentration of reactant A} 
(a) – log10[A] vs t
(b) – loge[A] vs t
(c) log10[A] vs log t
(d) [A] vs t

Answer   B

Question. T50 of first -order reaction is 10 min. Starting with 10 mol L–1, rate after 20 min is 
(a) 0.0693 mol L–1 min–1
(b) 0.0693 × 2.5 mol L–1 min–1
(c) 0.0693 × 5 mol L–2 min–1
(d) 0.0693 × 10 mol L–1 min–1

Answer   B

Question. The first order rate constant for a certain reaction increases from 1.667 × 10–6 s–1 at 727ºC to 1.667 × 10–4 s–1 at 1571ºC. The rate constant at 1150ºC, assuming constancy of activation energy over the given temperature range is
[Given : log 19.9 = 1.299] 
(a) 3.911 × 10–5 s–1
(b) 1.139 × 10–5 s–1
(c) 3.318 × 10–5 s–1
(d) 1.193 × 10–5 s–1

Answer   C

Question. In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason that
(a) collision frequency increases by a factor of 2 to 3.
(b) fraction of molecules possessing threshold energy increases by a factor of 2 to 3
(c) Activation energy is lowered by a factor of 2 to 3.
(d) none of these

Answer   B

Question. The rate constant for the reaction, 2N2O5 →4NO2 +O2 is 3.0x10-4 s-1 . If start made with 1.0 mol L–1 of N2O5, calculate the rate of formation of NO2 at the moment of the reaction when concentration of O2 is 0.1 mol L–1.
(a) 2.7 x10-4 molL-1s-1 
(b) 2.4x10-4  molL-1s-1
(c) 4.8x10-4  molL-1s-1
(d) 9.6x10-4  molL-1s-1

Answer   D

Question. A reaction which is of first order w.r.t. reactant A, has a rate constant 6 min–1. If we start with [A] = 0.5 mol L–1, when would [A] reach the value of 0.05 mol L–1
(a) 0.384 min
(b) 0.15 min
(c) 3 min
(d) 3.84 min

Answer   A

Question. Half-lives of a first order and a zero order reaction are same. Then the ratio of the initial rates of first order reaction to that of the zero order reaction is 
(a) 1/0.693
(b) 2 × 0.693
(c) 0.693
(d) 2/0.693

Answer   B

Question. Collision theory is used to explain how chemical species undergo a reaction. Using this theory and the kinetic molecular model, which of the following does NOT influence the rate of a chemical reaction?
(a) The temperature of the system
(b) The geometry or orientation of the collision
(c) The velocity of the reactants at the point of collision
(d) All of the above influence the rate

Answer   D

Question. For the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g), the rate law is: Rate = k [NO2]2.
If 0.1 mole of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?
(a) Both k and the reaction rate remain the same
(b) Both k and the reaction rate increase
(c) Both k and the reaction rate decrease
(d) Only k increases, the reaction rate remain the same

Answer   A


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