Asked by Blessing
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.
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.
Answers
Answered by
DrBob222
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.
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.
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