A1.50-kg iron horseshoe initially at 590°c is dropped into a bucket containing 17.0 kg of water at 24.0°c. what is the final temperature of the water–horseshoe system? ignore the heat capacity of the container and assume a negligible amount of water boils away.

29.3  °C

Explanation:

= mass of iron horseshoe = 1.50 kg

= Temperature of iron horseshoe initially = 590 °C

= specific heat of iron = 450 J/(kg °C)

= mass of water = 17 kg

= Temperature of water initially = 24.0 °C

= specific heat of water = 4186 J/(kg °C)

= Final equilibrium Temperature

using conservation of heat

Heat lost by iron horseshoe = Heat gained by water

= 29.3  °C

i think the answer would be reserve.