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Chemistry
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13 Dec 2019

(A) C3H8 (g) + O2 (g) ® CO2 (g) + H2O (g)

(b) C3H8 (g) + O2 (g) ® CO2 (g) + CO (g) + H2O (g)

The equation presented above shows (a) combustion of propane with abundant oxygen and (b) incomplete combustion of propane when oxygen availability is limited. Use these equations to answer the following questions.

Balance both equations

How much carbon monoxide (g) will be produced after burning a 20-pound propane tank with a limited access to oxygen (incomplete combustion)?

Calculate the heat released (enthalpy of reaction) for each reaction if an entire 20-pound propane tank is used?

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Bunny Greenfelder
Bunny GreenfelderLv2
17 Dec 2019

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Related questions

24.​Limiting Reagent problems, including Stoichiometry, Actual yield, Theoretical yield and Percent yield.

​A. I react 5.0 grams of propane, C3H8, with excess oxygen to produce water and carbon dioxide. Produce the balanced combustion equation of propane and determine the theoretical yield of water. If only 6.8 grams of water are produced what is the percent yield of water?

B. A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reagent and how much excess reactant remains on completion of the reaction? What is the theoretical yield of NO. The equation below represents this reaction. ____ NH3(g) + ____ O2(g) ® ____ NO(g) + ____ H2O(g)

​C. If 23.54 grams of nitrogen is reacted with 11.14 grams of hydrogen. Balance the following reaction. What is the theoretical yield of this reaction and which component is the limiting reagent? If only 8.26 grams of ammonia are produced what is the percent yield? ____ N2(g) + ____ H2(g) ® ____ NH3(g)

Propane (C3H8) is a common gas used for generating flames for cooking and camping. It undergoes a combustion reaction with excess oxygen (O2) to yeld carbon dioxide (CO2), Water (H2O) and heat. Suppose that you only have 82g propane for your trip.

A) Write the balanced stoichiometric reaction for the combustion of propane.

B) For every molecule of CO2, what is the mass percentage of C?

C) Suppose that your torch has a fixed amount of oxygen at 50g. What is the limiting reagent for your reaction and how many mols of water are produced if this reactant is consumed completely?

D) How much of the excess reagent is remaning after burning up all of the limiting reagent above?

E) Based on the chemistry described above, explain why somethering a fire puts a flame out.

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

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