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Chapter 3: Problem 71

The combustion of one mole of liquid ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) , produces 1367 \(\mathrm{kJ}\) of heat. Calculate how much heat is produced when 235.0 \(\mathrm{g}\) of ethanol are combusted.

Short Answer

Expert verified
When 235.0 g of ethanol is combusted, 6971.7 kJ of heat is produced.

Step by step solution

01

Find the molar mass of ethanol

First, we need to find the molar mass of ethanol, CH3CH2OH. The molar mass of carbon is 12.01 g/mol, hydrogen is 1.01 g/mol, and oxygen is 16.00 g/mol. There are 2 carbon atoms, 6 hydrogen atoms, and 1 oxygen atom in ethanol. Molar mass of ethanol = ( 2 * 12.01 g/mol) + (6 * 1.01 g/mol) + 16.00 g/mol = 46.07 g/mol
02

Convert mass of ethanol to moles

Now that we have the molar mass of ethanol, we can convert the given mass of ethanol in grams to moles using the molar mass as a conversion factor. Moles of ethanol = \(\frac{235.0 \,\text{g}}{46.07 \,\text{g/mol}} \)= 5.10 moles
03

Calculate the heat produced

We know that the combustion of 1 mole of ethanol produces 1367 kJ of heat. Therefore, we can calculate the heat produced when 5.10 moles of ethanol are combusted by multiplying the moles of ethanol by the heat released per mole. Heat produced = 5.10 moles * 1367 kJ/mol = 6971.7 kJ When 235.0 g of ethanol is combusted, 6971.7 kJ of heat is produced.

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