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The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid barium hydroxide octahydrate:

2NH4Cl(s) + Ba(OH)2 x 8H2O(s)---->2NH3(aq)+BaCl2(aq)+10H2O(1)

The (triangle then an H) for this reaction is 54.8 kJ. How much energy would be absorbed if 23.7 g of NH4Cl reacts?

Answer :

Reaction is :
2NH4Cl(s) + Ba(OH)2 x 8H2O(s)---->2NH3(aq)+BaCl2(aq)+10H2O(1)
Delta H= 54.8kJ
Molar mass of NH4Cl = 53.5 g/mol
(23.7 g NH4Cl x (1 mol NH4Cl / 53.5 g NH4Cl) x (54.8 kJ / 2 mol NH4Cl) = 12.13 kJ

The energy that should be absorbed is 11.84 KJ

Calculation of energy:

The moles of NH4Cl is = 23.7 ÷ 54.8 = 0.432

Since Δ for this reaction is 54.8 kJ and there is 23.7 g

So, the energy should be

= 54.8 ÷ 2 × 0.432

= 11.84 KJ

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