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Problem 53 Medium Difficulty

Consider the thermochemical equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover:

If a bottle of nail polish remover contains 177 mL of acetone, how much heat is released by its complete combustion? The density of acetone is 0.788 g>mL.

Answer

$-4.30 \times 10^{3} \mathrm{kJ}$

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04:13

KC

Kevin C.

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Chemistry 102

Chemistry 101
Chemistry: Structure and Properties

Chapter 9

Thermochemistry

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Video Transcript

So in this case we want to know uh the heat release. We know that the heat of this reaction, ears negative 16 58 kg joules per more, Which means that this is essentially a eggs, a thermic reaction that his heat is released. Uh We also know that acetone C 386 oh the molecular weight of acetone is 12. Multiplied by three plus six plus 16, which is 58 grams promote. We also know that the density of hesitant. Yeah, is also given. And that is .7 18g. uh, grams for more. Yeah. Sorry, this was grams. Yeah. So grams per milliliters. Sorry, .788 g for Miller leader. So, we know that we had 143. So one minute 43 mm Multiplied by 5.788 grants familiar leader will give us the weight of attitude, which is And in 12.68 g. Okay, if we divide this, we will get modes of acetone mhm. As 112.68, Divided by 58 molecular weight should give us 1.943. Okay, moles of Saskatoon. So now we know that this amount of a stone is reacting in order to form the in order to is taking part in the reaction. So we know that the heat generated is equal to the heat of the reaction, which was 1658, multiplied. Killer jewels multiplied. Let me put that a unit here, killer jewels for more, Multiplied by 1.943 moles. So that means the amount of heat release is 32-1.2 kilo jew. So that is the answer.

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