According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 975 kJ of energy?
SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ
AP Chem HW?
2017-02-08 12:25 pm
回答 (1)
2017-02-08 12:41 pm
SiO₂(s) + 4 HF(g) → SiF₄(g) + 2 H₂O(l) …. ΔH°rxn = -184 kJ
Refer to the above equation. 2 moles of H₂O is formed when 184 kJ of heat is produced.
When 975 kJ of energy is produced, no. of moles of H₂O formed = [(2 mol) / (184 kJ)] × (975 kJ) = 10.6 mol
Molar mass of H₂O = (1.0×2 + 16.0) g/mol = 18.0 g/mol
When 975 kJ of energy is produced, mass of H₂O formed = (10.6 mol) × (18.0 g/mol) = 191 g (to 3 sig. fig.)
Refer to the above equation. 2 moles of H₂O is formed when 184 kJ of heat is produced.
When 975 kJ of energy is produced, no. of moles of H₂O formed = [(2 mol) / (184 kJ)] × (975 kJ) = 10.6 mol
Molar mass of H₂O = (1.0×2 + 16.0) g/mol = 18.0 g/mol
When 975 kJ of energy is produced, mass of H₂O formed = (10.6 mol) × (18.0 g/mol) = 191 g (to 3 sig. fig.)
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