What is the enthalpy change in $kJ$ when $1$ gram-equivalent of a strong base reacts with an excess of a strong acid?

The enthalpies of neutralization of $HCN$ and $H_2S$ with a strong base are $12.13 \ kJ \ equi^{-1}$ and $15.9 \ kJ \ equi^{-1}$ respectively. Then:

For the reaction $NH_4^+ + S^{2-} \rightleftharpoons NH_3 + HS^-$,identify the nature of $NH_3$ and $HS^-$ in the context of the Brønsted-Lowry theory.

$A$ $Lewis$ acid is a substance that:

Identify the strongest base according to the Bronsted-Lowry theory from the following.

An acid is a compound which furnishes ($Bronsted-Lowry$ concept):