Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R.
Assertion A : $H_{2} Te$ is more acidic than $H_{2} S$ .
Reason R: Bond dissociation enthalpy of $H_{2} Te$ is lower than $H_{2} S$ .
In the light of the above statements. Choose the most appropriate from the options given below.

Question

Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R.

Assertion A : $H_{2} Te$ is more acidic than $H_{2} S$ .

Reason R: Bond dissociation enthalpy of $H_{2} Te$ is lower than $H_{2} S$ .
In the light of the above statements. Choose the most appropriate from the options given below.

Aicharya · Accepted Answer

Bond enthalpy, also referred to as bond energy or bond dissociation energy, is the energy required to break a particular covalent bond in one mole of molecule in a gaseous state.
The bond dissociation enthalpy of $H_{2} Te$ is lower than that of $H_{2} S$ .
As a result, less energy is required to break the $H_{2} Te$ bond, releasing ${[H]}^{+}$ is easier, and the acidity of $H_{2} Te$ is greater.
$H_{2} S$ , on the other hand, has a high bond dissociation energy and so has lower acidity.
Hence, Both A and R are true and R is the correct explanation of A.

Given below are two statements: One is labelled as Assertion A and the other is labelled as Reason R.…

Solution