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

Question

(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?

Explanation / Answer

I have a doubt in the part of the heat and enthalpy, but here's the other two part:

Balanced equations:
C3H8(g) + 5O2(g) ------> 3CO2(g) + 4H2O(g)

C3H8(g) + 4O2(g) --------> CO2(g) + 2CO(g) + 4H2O(g)

For the second part, let's convert the pound to grams, and use the molecular weight of propane to get the moles:
m = 20 pounds * 453.59 g/pound = 9071.8 g
moles = 9071.8 / 44 = 206.18 moles

The mole ratio between propane and CO is 1:2 so the moles and mass of CO is:
mCO = 206.18 * 2 * (28) = 11546 g of CO

Hope this helps

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