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q (heat energy in Joules) = mass * specific heat * change in temp

1st problem:

q = (100 g H2O)(4.180 J/gC)(100 C - 50 C)

= 20900 Joules

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2nd problem:

q = (100 g H2O)(4.180 J/gC)(70 C - 60 C)

= 4180 Joules

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As you can see from 50 C to 100 C takes much more heat energy as one would intuitively think, 20900 J/4180 J = 5 times as much energy.

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Wiki User

12y ago
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Wiki User

7y ago

If by "boil" you mean have it all evaporate, that takes MUCH more energy. For example, to increase the temperature of one gram of water from 20 to 100 degrees Celsius, you need 4.2 joules/gram/degree times 80 degrees = about 336 joules; then, to evaporate all the water, you need an additional 2257 joules.

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Wiki User

13y ago

No, it obviously takes less energy because hot water is closer to the target temperature than warm or ice water.

Comment: see discussion page.

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Wiki User

8y ago

It takes more energy to heat the water than to boil it because, once you get to the boiling point you stay at the boiling point.

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Wiki User

7y ago

To boil it.

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Anonymous

Lvl 1
3y ago

kj'

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Q: Does it take more energy to heat the water to 100 degrees Celsius or to boil it?
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