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Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water that had been in the refrigerator at $3.8^{\circ} \mathrm{C},$ how much heat is needed to convert all of that water into sweat and then to vapor? (Note: Your body temperature is $36.6^{\circ} \mathrm{C} .$ For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water.)

$1.4 \times 10^{3} \mathrm{kJ}$

01:25

Aadit S.

Chemistry 102

Chapter 10

Liquids and Solids

Liquids

Solids

Carleton College

University of Central Florida

Rice University

Lectures

04:08

In physics, a solid is a s…

03:07

A liquid is a nearly incom…

04:14

Evaporation of sweat is an…

04:27

0:00

Evaporating sweat cools th…

01:36

00:58

01:29

01:42

The evaporation of perspir…

$\cdot$ Evaporative coolin…

02:03

Many species cool themselv…

04:10

Metabolic activity in the …

03:32

When you drink cold water,…

02:34

The excess internal energy…

01:47

Evaporation of sweat is th…

05:17

Water is used as the worki…

01:41

The latent heat of vaporiz…

03:34

06:23

In exercising, a weight li…

10:17

An athlete whose mass is 7…

02:48

For many years drinking wa…

11:55

phase transitions. The fasting we need to do in this podcast is convert the mass of 20 ounces of water into grams. About 20 ounces H 20 is equal to 5.7 times 10 to the power to grams of H 20 So now we calculate the heat required. Using Cuban is equal to M C Dub T, where Q one is equal to 7.8 times 10 to the four jewels. Firstly, he required to raise from 3.8 degrees C to 36.6 degrees C. So in the next step, we can calculate the moles of sweat that is present in this volume. So what we take is the fresh peach for a start, 5.7 times 10 to 2 g of sweat multiplied by one mole sweat divided by 18.15 g sweat that equals 31.6 mol. That's six miles of sweat. Then we calculate the he required vapor I sweat, which we can call YouTube people to models multiplied by Delta H. Vaporization, where Q two is 31.6, multiplied by 40.7 times 10 to the three jewels Permal Que two is therefore 1.29 times. Turn to the six jewels, and so it's calculate the total heat. We need to add these together the heat from the previous page. So on a fresh page, our total heat is 1.37 times 10 to the sixth jewels. Now we can convert this into killer jewels. It's approximately 1.4 times 10 to the 3 kg jewels.

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