When 91.5 g of isopropyl alcohol which has an empirical formula of C3H8O is burned in excess oxygen gas, how many grams of H2O are formed? MWC = 12.011 g/mol, MWH = 1.00794 g/mol, and MWO = 15.9994 g/mol.
1. 47.9229
2. 84.1255
3. 52.2617
4. 49.8948
5. 86.9152
6. 119.705
7. 88.0758
8. 76.2076
9. 62.9663
10. 109.729

Explanation:

This is a combustion reaction. The complete combustion of a hydrocarbon produces carbon dioxide and water.

The combustion reaction of isopropyl alcohol is represented by the balanced hemical equation:

Thus, 2 moles of produce 8 moles of .

1. Convert the 91.5 g of isopropyl alcohol into number of moles

2. Calculate the the number of moles of water produced using the mole ratio:

3. Convert to mass of water

So far, I have kept a large number of digits because these are intermediate calculations.

You should report the result with 3 significant figures, but all the answer choices contain more than that.

The last choice, 109.729, is the closest to the correct value.

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