Question

Give the data in table below, $\Delta$ H_rxn for the reaction.

NH₃(aq)+H₂SO₄(aq) $\rightarrow$ HSO₄^-(aq)+NH₄⁺(aq)

Compound /   $\Delta$ H_f (kj/mol)

NH₃= -80.29

H₂SO₄= -909.3

NH₄⁺= -132.5

HSO4- = -212.08

Answer 1

NH₃(aq)+H₂SO₄(aq) $\rightarrow$ HSO₄^-(aq)+NH₄⁺(aq)

$\Delta$ H_{rxn =} $\Delta$ H_{f products -} $\Delta$ H_{f reactants}

               = (- 212.08 - 132.5) - (- 80.29 - 909.3)

               = - 344.58 + 989.59

$\Delta$ Hrxn   = 645.01 kJ/mol