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Imagine that your water heater has broken, but you want to take a bath. You fill your bathtub with 25 kg of room-temperature water (about 25 C). You figure that you can boil water on the stove and pour it into the bath to raise the temperature.
How much boiling water would you need in order to raise the bath to body temperature (about 37C)? Assume that no heat is transferred to the surrounding environment.
I know this is a simple question, but I'm totally stuck.
I calculated the amount of heat needed to raise the temperature to 37C:
q=Cm \Delta{T}
=1*25000*12
=300 000 cal.
Since energy is conserved, I used the the same equation to calculate the mass of the boiling water. The mass just equals 25kg, which is totally wrong.
Can anyone help me out and point me in the right direction?
Thank you.
How much boiling water would you need in order to raise the bath to body temperature (about 37C)? Assume that no heat is transferred to the surrounding environment.
I know this is a simple question, but I'm totally stuck.
I calculated the amount of heat needed to raise the temperature to 37C:
q=Cm \Delta{T}
=1*25000*12
=300 000 cal.
Since energy is conserved, I used the the same equation to calculate the mass of the boiling water. The mass just equals 25kg, which is totally wrong.
Can anyone help me out and point me in the right direction?
Thank you.