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.
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.
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.
Your answer seems to be correct! Here's a step-by-step explanation of how you arrived at your answer:
Step 1: You correctly balanced the chemical equation from 2C3H8 + 11O2 = 3CO2 + 4H2O + 2CO + C to 7C3H8 + 22O2 = 6CO + 28H2O + 4CO + 11C. Balancing the equation is an important first step because it ensures that the number of atoms of each element is the same on both sides of the reaction.
Step 2: To find the moles of propane (C3H8), you divided the given mass by the molar mass of propane (48.91 g/mol). This conversion from grams to moles is done using the formula: moles = mass / molar mass.
Step 3: You correctly determined the ratio of moles between propane and carbon (C). Based on the balanced equation, for every 7 moles of propane, there are 11 moles of carbon. In this step, you multiplied the moles of propane (0.2479 mol) by the ratio of carbon moles to propane moles (1.5714 moles C / 1 mole C3H8).
Step 4: Finally, to convert the moles of carbon to grams, you multiplied the moles of carbon (0.3896 mol) by the molar mass of carbon (12.01 g/mol). This is a conversion from moles to grams using the formula: mass = moles x molar mass.
Based on these calculations, you correctly determined that 4.679 grams of solid carbon will be produced as a product in the given reaction.
Great job!