Question

The amount of boiling water required to raise the temperature of 25.0 kg of water in the bath to body temperature is 4.80 kg. In this process, the heat lost by the boiling water is equal to the heat gained by the room-temperature water. How much heat was transferred in this process?

Answer 1

Answer:

1,270,080 Joules

Explanation:

The specific heat of water is 4200J/kg

Body temperature 37°C

Boiling point of water 100°C

Using the common knowledge information as above...

Specific heat is the energy required to raise/decrease the temperature of 1 kg of substance by 1°C

Specific heat of water bring 4200J/kg, it requires to lose 4200*4.8*63 = 1,270,080 J to cool down 4.8 kg of boiling water from 100°C to body temperature of 37°C

Simply putting it in formula c= ∆E/(m*∆T)

E = 4200*4.8*63

E= 1,270,080

Also initial temperature of bath water can be found out in a similar way i.e 37–1,270,080/(4200*25)= 24.9°C

Please correct me if I'm wrong, cheers ! :)