Posted by **Will** on Tuesday, October 13, 2009 at 8:55pm.

Could someone please tell me if I did this question correctly?

An incomplete combustion reaction of 12.125 grams of propane proceeds as follows: 2C3H8 + 11O2 = 3CO2 + 4H2O + 2CO + C(s).How many grams of solid carbon residue are produced as a product?

my answer:

known:

molar mass of propane=48.91g/mol

molar mass of carbon= 12.01g/mol

Step 1)

The balanced chemical equation for "2C3H8 + 11O2 = 3CO2+ 4H2O + 2CO + C"

is "7C3H8 + 22O2 = 6CO + 284H2O + 4CO + 11C."

Step 2)

Convert 12.125 grams of propane to moles.

12.125g/(48.91g/mol)

=.2479mol

step 3)

The ratio of propane to carbon dioxide is 7:11(or 1 to 1.5714). Therefore, for every mole of propane there will be 1.5714mol of carbon.

1.5714(.2479mol)=.3896mol of carbon.

step 4)

Convert back to grams.

.3896mol( 12.01g/mol)

= 4.679g

Answer:

In the given reaction, 4.679g of solid carbon will be produced.

Thanks for your help.

- chemistry -
**DrBob222**, Tuesday, October 13, 2009 at 10:43pm
2C3H8 + 11O2 = 3CO2 + 4H2O + 2CO + C(s).

**The equation isn't balanced; therefore, any calculation based on an unbalanced equation will not be correct.
**

C balanced.

H does not. There are 16 atoms on the left and 8 on the right.

O does not. There are 22 atoms on the left and 12 on the right.

- chemistry -
**Will**, Wednesday, October 14, 2009 at 12:11am
In step 1), I balanced the equation to "7C3H8 +22O2 -->> 6CO2 + 28H2O +4CO +11C". Is this not correct, along with the rest of my answer?

Excuse the my typo in my original when I put the coefficient for H2O as 284 when it should be 28.

Thank you.

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