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Many portable gas heaters and grills use propane, C3H8(g), as a fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is completely combusted in air under standard conditions.

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Hubert Koch
Hubert KochLv2
23 May 2020

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Related questions

Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO2(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1 atm and 25 °C).

(a) coal, C(s, graphite);

(b) natural gas, CH4(g);

(c) propane, C3H8(g);

(d) octane, C8H18(l) (ΔHf° = –250.1 kJ ·mol–1)

UNITS: mol * MJ^-1

Propane is often used as a home fuel in areas where natural gas is not available. When 3.00 grams of propane (C3H8 (g)) are burned in excess oxygen in a bomb calorimeter that has a total heat capacity of 32.7 kJ/K, the temperature of the calorimeter increases by 4.25 K.

a.) Calculate the heat of the calorimeter, qCal. (HINT: Units should be in kJ.)

b.) Calculate, by using the First Law of Thermodynamics, the heat of the reaction, qrxn.

c.) Assuming that ΔE ≈ ΔH, calculate the standard enthalpy of combustion in (i) kilojoules per gram of propane, and (ii) kilojoules per mole of propane.

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