Problem: The propane fuel (C3H8) used in gas barbeques buns according to the following thermochemical equation: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)    ΔH°rxn = -2217kJ If a pork roast must absorb 1600 kJ to fully cook, and if only 12% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast? Express your answer using two significant figures.

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The propane fuel (C3H8) used in gas barbeques buns according to the following thermochemical equation: 

C3H(g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)    ΔH°rxn = -2217kJ 

If a pork roast must absorb 1600 kJ to fully cook, and if only 12% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast? Express your answer using two significant figures.

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