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Naddika [18.5K]
2 years ago
7

You drink part of your bottle of water, leaving 160 g in the bottle. When you purchased the water, it had a temperature of 10oC.

After carrying the bottle around for awhile, you take a sip and find that the water is an unpleasantly warm 35oC. How much heat energy did the water left in the bottle absorb? Water has a specific heat capacity of 4.2 J/(g * oC).
Chemistry
1 answer:
Evgesh-ka [11]2 years ago
7 0

The energy that the water in the  bottle absorbed is obtained as 16800 J.

<h3>What is the specific heat capacity?</h3>

The specific heat capacity of the water refers to the energy that is required to raise the temperature of 1Kg of the water by 1 degree.

Now we have the following;

mass (m) =  160 g

temperature change dT = ( 35oC -  10oC)

specific heat capacity (c)= 4.2 J/(g * oC).

Now;

H = mcdT

H =  160 g * 4.2 J/(g * oC) *  ( 35oC -  10oC)

H = 16800 J

Learn more about specific heat capacity:brainly.com/question/1747943

#SPJ1

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