NEET Chemistry Chemical Kinetics Questions Solved

BOARD

For a decompostion reaction, the values of k at two different temperatures  are given below :

K1 =2.15 ×10-8 L mol-1s-1 at  650 K

K2 =2.39 ×10-7 L mol-1s-1 at 700 K

Calculate the value of activation energy for this reaction.

(R= 8.314 J K-1 mol-1)(Log 11.11 =1.046)

1.182.2 kJ

2. 152.7 kJ

3.200.4 KJ

4.NONE

Given : K1 =2.15 ×10-8 L mol-1s-1 , T1= 650 K

           K2 =2.39 ×10-7 L mol-1s-1 , T2= 700 K

           R= 8.314 J K-1 mol-1                     Ea = ?

According to formula: log k2k1=Ea2.303RT2-T1T1T2  

                 or       log2.39 ×10-72.15×10-8=Ea2.303×8.314700-650700×650  

                 or       log 1.111× 10 =Ea19.14750455000  

                  or       log 1.111+ log10 =Ea19.14750455000  

                 or       0.0457 +1 =Ea19.147×19100

                or   Ea = 1.0457×19.147×9100

               Ea = 1,82,200.36 J =182.20 KJ

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