Chemical Kinetics Test

Result

Chemical Kinetics Test - 19

Score
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Rank
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Weekly Quiz Competition

Question 1
4 / -1

What will be the order of the reaction if doubling the concentration of a reactant increases the rate by a factor of 4 and trebling the concentration of the reactant by a factor of 9 ?

A
1

B
2

C
3

D
0
Question 2
4 / -1

If the half time for a particular reaction is found to be constant and independent of the initial concentration of the reactants then reaction is of ...

A
1

B
2

C
3

D
0
Question 3
4 / -1

The rate of reaction A + B + C → Products is given by r = K[A][B]^o[C]. If A is taken in large excess, the order of the reaction would be

A
0

B
1

C
2

D
nil
Question 4
4 / -1

For a reaction 2A + B → Products, the active mass of B is kept constant and that of A is doubled. The rate of reaction will then

A
increase two times

B
increase four times

C
decrease two times

D
decrease four times
Question 5
4 / -1

The conversion of A → B follows second order kinetics. Doubling the concentration of A will increase the rate of formation B by a factor of

A
1⁄4

B
2

C
1⁄2

D
4
Question 6
4 / -1

Ethyl acetate is hydrolysed in alkaline medium, its order of a reaction and molecularity are respectively

A
1, 1

B
1, 2

C
2, 1

D
2, 2

Solution
Question 7
4 / -1

The given reaction 2FeCl₃ + SnCl₂ → 2FeCl₂ + SnCl₄ is an example of ________ reaction

A
first order

B
second order

C
third order

D
none of these
Question 8
4 / -1

If concentration of reactants is increased by ‘x’, then rate constant K becomes ..

A

B

C
k + x

D
k
Question 9
4 / -1

The rate constant is given by equation K = p.z.e^-Ea/RT which factor should register a decrease for the reaction to proceed more rapidly ?

A
E

B
T

C
Z

D
P
Question 10
4 / -1

The time for half life of a certain reaction A → Products, is one hour. When the initial concentration of the reactant A is 2 mol L^-1 how much time does it take for its concentration to come from 0.50 to 0.25 mole L^-1 if it is a zero order reaction ?

A
0.25 h

B
1 h

C
4 h

D
0.5 h

Solution