CBSE TEST PAPER-03 CLASS - XII CHEMISTRY (Chemical Kinetics), CBSE Class 12 Notes | EduRev

Class 12 : CBSE TEST PAPER-03 CLASS - XII CHEMISTRY (Chemical Kinetics), CBSE Class 12 Notes | EduRev

 Page 1


CBSE TEST PAPER-03 
CLASS - XII CHEMISTRY (Chemical Kinetics) 
Topic: -Determination of order of a reaction. 
1. Identify the reaction order for from each of the following rate constant –
a) k = 2.3 ×10
-5
 L mol-1 s
-1
b) k = 3.1 × 10
-4
 s
-1
[1] 
2. Consider the equation 2 NO (q) + 2H 2 (g) ? N 2 (g) + 2H 2O (g)
The rate law for this equation is first order with respect to H 2 and second
order with respect to NO. write the rate law for this reaction. [1] 
3. The rate Law for the reaction A+B ? C is rate = K [A]
2
 [B] . What would the
reaction rate be when concentration of both  A and B are doubled? [2] 
4. Write the integrated rate equation for –
i) zero order reaction.
ii) first order reaction. [2] 
5. From the graph below [2] 
i) Identify the order of reaction.
ii) What will be the unit of rate constant?
Page 2


CBSE TEST PAPER-03 
CLASS - XII CHEMISTRY (Chemical Kinetics) 
Topic: -Determination of order of a reaction. 
1. Identify the reaction order for from each of the following rate constant –
a) k = 2.3 ×10
-5
 L mol-1 s
-1
b) k = 3.1 × 10
-4
 s
-1
[1] 
2. Consider the equation 2 NO (q) + 2H 2 (g) ? N 2 (g) + 2H 2O (g)
The rate law for this equation is first order with respect to H 2 and second
order with respect to NO. write the rate law for this reaction. [1] 
3. The rate Law for the reaction A+B ? C is rate = K [A]
2
 [B] . What would the
reaction rate be when concentration of both  A and B are doubled? [2] 
4. Write the integrated rate equation for –
i) zero order reaction.
ii) first order reaction. [2] 
5. From the graph below [2] 
i) Identify the order of reaction.
ii) What will be the unit of rate constant?
6. The reaction 2N 2O 5 (g) ? 2NO 2 (g) +O 2 (g) was studied and the following data were
collected :
s.no [N 2O 5] mol L
-1  
Rate of disappearance of [N 2O 5]
(mol/L/min 
1.  1.13×10
-2
  34×10
-5
 
2.  0.84 ×10
-2
  25×10
-5
 
3.  0.62×10
-2
  18×10
-5
Determine 
i) The order
ii) The rate law.
iii) Rate constant for the reaction. [3] 
7. The following experimental data was collected for the reaction:
Cl 2 (g) + 2NO (g) ? 2 NOCl(g)
Trial  Intial conc. Of Cl 2 (mol/L)  [NO] mol/L   Initial Rate,(mol/L/s) 
1  0.10  0.010  1.2 X 10
-4
 
2  0.10  0.030  10.8 X 10
-4
3  0.20  0.030  21.6 X 10
-4
 
Construct the rate equation for the reaction. [3] 
8. Draw a graph for
a) Concentration of reactant against time for a zero order reaction.
b) Log [Ro]/ [R] against time for a first order reaction. [2] 
9. What is the use of integrated rate equation? [2] 
10. For first order reaction –
A ? B
Write      (1) Differential rate law. 
 (2) Integrated rate law. [2] 
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