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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).

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

What is the specific heat capacity?

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:https://brainly.com/question/1747943

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