Could someone please tell me if I did this question right?
An incomplete 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:
Step 1)
Balanced the given chemical equation:
2C3H8 + 11O2=3CO2+ 4H2O + 2CO + C
=7C3H8 + 19O2=6CO + 28H2O + 4CO + 11C
Step 2)
Convert 12.125 grams of propane to moles:
12.125g/(44.0956g/mol)
=.27497mol
step 3)
The ratio of propane to carbon is 7:11(or 1 to 1.5714). Therefore, for every mole of propane there will be 1.5714 moles of carbon.
1.5714(.27497mol)=.41630mol of carbon.
step 4)
Convert back to grams.
.41630mol(12.0107g/mol)
= 5.0000g
Answer:
In the given reaction, 5.0000g of solid carbon will be produced.
Thanks for your help.
correct
Thank you.
I have news for you. The equation you wrote isn't balanced; therefore, if you have the right answer it is only because the coefficients just happened to work out that way.
To verify if your answer is correct, let's go through the steps and calculations you've done.
Step 1:
You have correctly balanced the chemical equation.
Step 2:
You have correctly converted the given mass of propane (12.125g) to moles. The molar mass of propane (C3H8) is 44.0956g/mol. So, your calculation is correct.
Step 3:
You have correctly determined the ratio of moles of propane to moles of carbon. The ratio is 7:11, or approximately 1:1.5714. You have multiplied this ratio by the moles of propane you calculated in step 2.
Step 4:
You have correctly converted the moles of carbon to grams using the molar mass of carbon (12.0107g/mol).
Your answer, 5.0000g of solid carbon, seems to be correct.
Overall, your calculations and steps are accurate, and you have obtained the correct answer. Well done!