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?
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.
To calculate each of these values, you will need to follow a few steps:
a) How much heat energy is produced by the combustion of 1000.0 grams of isopropyl alcohol?
1. Calculate the number of moles of isopropyl alcohol using its molar mass (60.1 g/mole) and the given mass (1000.0 grams).
Number of moles = Mass / Molar mass
2. From the balanced equation, you know that 1 mole of isopropyl alcohol produces 4012 kJ of heat energy. Multiply this value by the number of moles of isopropyl alcohol calculated in step 1 to find the heat energy produced.
Heat energy = Number of moles of isopropyl alcohol * 4012 kJ
b) To completely combust 1,000.0 grams of isopropyl alcohol, what weight in grams of oxygen is needed?
1. Calculate the number of moles of isopropyl alcohol using its molar mass (60.1 g/mole) and the given mass (1000.0 grams).
Number of moles of isopropyl alcohol = Mass / Molar mass
2. From the balanced equation, you know that the ratio between isopropyl alcohol and oxygen is 1:9. Multiply the number of moles of isopropyl alcohol calculated in step 1 by the ratio to find the moles of oxygen required.
Moles of oxygen = Number of moles of isopropyl alcohol * 9
3. Calculate the mass of oxygen using its molar mass (32.0 g/mole) and the moles of oxygen calculated in step 2.
Mass of oxygen = Moles of oxygen * Molar mass
c) What weight in grams of carbon dioxide is formed when 1,000.0 grams of isopropyl alcohol is completely combusted?
1. Calculate the number of moles of isopropyl alcohol using its molar mass (60.1 g/mole) and the given mass (1000.0 grams).
Number of moles of isopropyl alcohol = Mass / Molar mass
2. From the balanced equation, you know that the ratio between isopropyl alcohol and carbon dioxide is 1:6. Multiply the number of moles of isopropyl alcohol calculated in step 1 by the ratio to find the moles of carbon dioxide produced.
Moles of carbon dioxide = Number of moles of isopropyl alcohol * 6
3. Calculate the mass of carbon dioxide using its molar mass (44.0 g/mole) and the moles of carbon dioxide calculated in step 2.
Mass of carbon dioxide = Moles of carbon dioxide * Molar mass
These steps will guide you in setting up the calculations for each question. Once you have the equations set up, you can substitute the values and calculate the answers.