Acetylene gas (ethyne; HC?CH) burns in an oxyacetylene torch to produce carbon d

Question

Acetylene gas (ethyne; HC?CH) burns in an oxyacetylene torch to produce carbon dioxide and water vapor, and the heat needed to weld metals. The heat of reaction for the combustion of acetylene is -1259 kJ/mol.
(a) Calculate the C?C bond energy, and compare your value with that in the table.
_______ kJ/mol

(b) When 375.0 g of acetylene burns, how many kilojoules of heat are given off?______ kJ

(c) How many grams of CO2 form?
______ g

(d) How many liters of O2 at 298 K and 18.5 atm are consumed?
______ L

Explanation / Answer

a)839 kJ/mol b)375g/(26g/mol) * 1259 kJ/mole = 18,160 kJ of energy c) 375g/(26g/mol) * 2 moles CO2/mole acetylene * 44g CO2/mole = 1269 g of CO2 d) 375/26 * 5/2 = 36.05 moles of O2 V = nRT/P = 36.05 *0.08206 * 298/18.5 = 47.66 Liters of oxygen consumed

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