2NH4Cl(s)+Ba(OH)2⋅8H2O(s)→2NH3(aq)+BaCl2(aq)+10H2O(l) The ΔH for this reaction is 54.8 kJ . How much energy would be absorbed if 24.7 g of NH4Cl reacts?
1 answer:
1) Chemical equation <span>2NH4Cl(s)+Ba(OH)2⋅8H2O(s)→2NH3(aq)+BaCl2(aq)+10H2O(l)
2) Stoichiometric ratios 2 mol NH4Cl(s) : 54.8 KJ3) Convert 24.7 g of NH4Cl into number of moles, using the molar mass molar mass of NH4Cl = 14 g/mol + 4*1 g/mol + 35.5 g/mol = 53.5 g/mol number of moles = mass in grams / molar mass number of moles = 24.7 g / 53.5 g/mol = 0.462 moles4) Use proportions: 2 moles NH4Cl / 54.8 kJ = 0.462 moles / x => x = 0.462 moles * 54.8 kJ / 2 moles = 12.7 kJ Answer: 12.7 kJ </span>
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