(a) A first order reaction is 50\; ^{o}/_{o} complete in 30 minutes at 300\; K and in 10 minutes at 320\; K. Calculate activation energy (E_{a}) for the reaction. (R=8.314\; J\; K^{-1}\; mol^{-1})

(b) Write the two conditions for collisions to be effective collisions.

(c) How order of reaction and molecularity differ towards a complex reaction ?

[Given : log2=0.3010,\; log3=0.4771,\; log4=0.6021,\; log5=0.6991]

 

 
 
 
 
 

Answers (1)

a) k = 0.693/ t1/2

k1= 0.693/ t1/2= 0.693 / 30

k2= 0.693/ t1/2= 0.693 / 10

log k2/k1 = Ea /2.303 R (1/ T1 -1/ T2)

log 3 = Ea /2.303 x 8.314 (1/ 300 -1/ 320)

Ea =  43.8 kJ/mol

b) Conditions for collisions to be effective collisions

1. Proper orientation and

2. Energy of the colliding particles should be more than threshold energy

c) For a complex reaction, order of reaction is applicable while molecularity has no meaning.

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