Question

The village blacksmith dunks a red-hot horseshoe into a large bucket of 22.0°C water. How much heat was lost by the horseshoe in vaporizing 0.0100 kg of water?

Answer 1

Answer:

25776J

Explanation:

Recall that heat lost/gained is obtained from

H=mcθ

H= heat lost/gained

m= mass of water = 0.0100 kg

c= 4200 J/kg°C

θ = temperature

Heat gained by the water in rising to 100°

H=  0.0100 * 4200 * (100-22)

H= 3276 J

Latent heat of vaporization of water = mL

Latent heat of vapourization = 0.0100*(22.5*10^5)=22500J

Heat lost by iron = heat gained by water

total heat gained by water =

22500+3276=25776J