Question

A freshly-forged iron horseshoe, with a mass of 0.399 kg is dropped into a 0.234 kg iron pot which contains 1.27 kg of water at 20.1 ^oC.

After the horseshoe, pot and water reach thermal equilibrium they have a temperature of 29.6 ^oC.

1. Assuming the pot and the water was in thermal equilibrium before the horseshoe entered the water, calculate the combined amount of heat gained by the pot and water as they cool the horseshoe.

2. Calculate the initial temperature of the horseshoe, giving your final answer in units of Kelvin.You should assume that no heat was lost to the environment and that the pot and the water were in thermal equilibrium before the horseshoe entered the water.Recall that the mass of the iron horseshoe was 0.399 kg, and the final temperature of the horseshoe is 29.6 ^oC. Give your answer in Kelvin.

Answer 1

Using the concept of energy conservation

Heat released by horsehoe = heat gain by watter + heat gain by pot

specific heat capacity of the Iron (c_I) = 0.444 kcal/Kg0C

specific heat capacity of the water (c_w) = 4.184 kcal/Kg.0C

Part 1

Combine heat gain by the pot and the water is

This gain in heat has to be come from the horseshoe due to its temprature dicrease.

using these value we can write

or

So the initial temprature of the horseshoe is 593.27 K