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Q

Consider the given plot of enthapy of the following reaction between A and B .

$A+B\rightarrow C+D$

Identify the incorrect statement .

• Option 1)

Activation enthapy to form C is $5\:kJmol^{-1}$ less than that to form D.

• Option 2)

C is the thermodynamically stable product.

• Option 3)

D is kinetically stable product .

• Option 4)

Formation of A and B from C has highest enthaply of activation .

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Activation Energy -

The minimum kinetic energy that reactants must have in order to form products.

- wherein

Description:

E.g.: In a gas phase reaction numerous collisions take place but only a tiny proportion which has sufficient energy to cross the energy barrier leads to product formation.

EC (activation energy of C) = (20-5)kJ mol- = 15 kJ mol-

E( activation energy of D) = (15-5)kJ mol- = 10 kJ mol-

activation energy of C is 5 kJ mol- more than that of D.

Option 1)

Activation enthapy to form C is $5\:kJmol^{-1}$ less than that to form D.

Option 2)

C is the thermodynamically stable product.

Option 3)

D is kinetically stable product .

Option 4)

Formation of A and B from C has highest enthaply of activation .

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