The standard enthalpy change for the combustion of 1 mole of propane is –2043.0 kJ.
What is the ΔH for the combustion of propane C3H8 at standard conditions?
The heat of combustion of propane, C3H8, as described in the equation C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l), is –2220 kJ mol-1 and the heats of formation of carbon dioxide gas and water liquid are –393.5 kJ mol-1 and -285.8 kJ mol-1 respectively.
What is the value of ΔH for the combustion of one mole of methane?
The combustion of methane, CH4, releases 890.4 kJ/mol. That is, when one mole of methane is burned, 890.4 kJ are given off to the surroundings. This means that the products have 890.4 kJ less than the reactants.
What is the complete combustion of propane?
The ideal combustion ration (“complete combustion”) for propane is 1 part propane (4%) to 24 parts of air (96%). Even at this ideal ration, combustion products, known as flue gases, still occur. However, under this scenario, those products are harmless carbon dioxide and water.
How do you calculate the combustion of propane?
The balanced chemical equation for the combustion of propane is: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g).
How many moles of propane are burned?
The molar mass of propane is 44 g/mole, so burning propane will release (2030kJ/mole) / (44g/mole) = about 46 kJ/g of fuel burned.
ANSWERS TO HOMEWORK #1 – THE WHOLE THING.
|kJ released per gram of fuel used||51||46|
How much energy is released when 0.2 mol of propane are burnt?
The energy released = (-2220 KJ/mol x 0.2 mol) / (1.0 mol) = -444.0 KJ/mol.
Which is the net energy released on complete combustion of propane?
Which is the net energy released on complete combustion of propane? –2024 kJ/mol.
How do you calculate delta H?
Subtract the sum of the heats of formation of the reactants from that of the products to determine delta H: delta H = –110.53 kJ/mol – (–285.83 kJ/mol) = 175.3 kJ.