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11 Dec 2019

Propane (C3H8) is burned according to the balanced chemical equation below. What mass of CO2 is emitted when enough propane is burned to generate 1.60 x 103 kJ of heat? C3H8 (g) + 5O2 (g) -> 3CO2 (g) + 4H2O (g)

A 25 g sample of gold absorbs 23.5 J of heat. If the initial temperature of the gold is 27 degrees Celsius, then what is the final temperature of the gold sample? (specific heat capacity of gold = 0.128 J/gK)

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Jean Keeling
Jean KeelingLv2
13 Dec 2019

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Related questions


A 16.0 gram sample of propane gas (C3H8) is burned according to the equation C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g).

In an enclosed container with a volume of 2.25L at a temperature of 322K.

If the sample of propane burns completely and no oxygen remains in the container, calculate the mole fractions of CO2 and H2O.

Calculate the total pressure in the container after the reaction.

Calculate the partial pressure of CO2 and H2O in the container after the reaction.

If 12.1 grams of propane is burned in the presence of 10.2 atm of oxygen at the above temperature and volume conditions, determine the theoretical yield of H2O.

The propane fuel (C3H8) used in gas barbeques burns according to the following thermochemical equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2217kJ. If a pork roast must absorb 1700 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?

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