Too bad. I'm ready for pork roasts.
C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (l) ΔrH = -2220 kJ/mol
We know that 3 moles CO2 are produced from 2220 kJ reaction. 1 mol CO2 = 44 g and 3 mols = 3*44 = 132 g so
132 g CO2 x (129 kJ/2220 kJ) = grams CO2 from 129 kJ of the above reaction of C3H8.
A propane BBQ combusts propane as shown below:
C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (l) ΔrH = -2220 kJ/mol
What mass of carbon dioxide (in g) is produced when a BBQ grill releases 129 kJ of heat to its surroundings at constant pressure?
No pork roasts were cooked in the making of this question.
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