First, the equation you have written is not balanced. Here is the corrected version.
2C2H8O + 7O2 (g) -> 4CO2 (g) 8H2O (l) + 4012 kJ of heat energy
a. You can look at this two ways. The bottom line is that 2*60.1 g alcohol releases 4012 kJ heat. So what will 1000 g release. You can do ratio/proportion; which is
(2*60.1/4012 kJ) = (1000 g/x) and solve for x grams. Or you can use dimensional analysis to obtain
q = (4012 kJ/2*60.1g) x 1000 = ?
b. This is a stoichiometry problem.
mols alcohol = grams/molar mass = ?
using the coefficients in the balanced equation, convert mols alcohol to mols O2.
Now convert mols O2 to grams. g O2 = mols O2 x molar mass O2 = ?
c. This done the same way as part b. You know mols alcohol, convert that to mols CO2 and convert that to grams CO2.
Post your work if you get stuck. BTW, I can't believe you posted that "balanced equation" this way because you can check it and see that it isn't balanced.
Note- I do not want the answers. I just need to know how to set up each..
The combustion of isopropyl alcohol (Molar Mass=60.1 g/mole) is described by the following balanced equation:
1 C2H8O + 9 O2 (g) -> 6 CO2 (g) 8H2O (l) + 4012 kJ of heat energy
a) How much heat energy is produced by the combustion of 1000.0 grams of isopropyl alcohol?
b) To completely combust 1,000.0 grams of isopropyl alcohol, what weight in grams of oxygen (Molar mass=32.0 g/mole) is needed?
c) What weight in grams of carbon dioxide (molar mass=44.0 g/mole) is formed when 1,000.0 grams of isopropyl is completly combusted?
1 answer