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d1i1m1o1n [39]
3 years ago
9

What is the final temperature of a sample of water if 12.15J of energy is added to 475g of water at an initial temperature of 20

.5°c?
Chemistry
1 answer:
VikaD [51]3 years ago
6 0

Answer:

The final temperature of water is <u>20.5061 °C.</u>

Explanation:

Let the final temperature of water be 'x'.

Given:

Heat added to water is, Q_{in}=12.15\ J

Initial temperature of water is, T=20.5\ \°C

Mass of water is, m=475\ g

Now, heat  is added to water and its temperature is increased. The temperature is increased because water absorbs all the heat.

Heat absorbed by water is given as:

Q_{abs}=mc(x-T) where 'c' is specific heat capacity of water and its value is equal to 4.186 J/g °C.

Now, plug in the given values and simplify.

Q_{abs}=475\times4.186\times(x-20.5)\\Q_{abs}=1988.35(x-20.5)

Now, from law of conservation of energy, we know that:

Heat absorbed by water = Heat added to water

Q_{abs}=Q_{in}\\1988.35(x-20.5)=12.15\\x-20.5=\frac{12.15}{1988.35}\\x-20.5=0.0061\\x=20.5+0.0061=20.5061\ \°C

So, the final temperature of water is 20.5061 °C.

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Substituting values;

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