Question

A 2-kg piece of iron is heated to 100°C, and then submerged in 2 kg of water initially at 0°C. The iron cools and the water warms until they are at the same temperature (in thermal equilibrium). Assuming there is no other transfer of heat involved, is the final temperature closer to 0°C, 50°C, or 100°C?

Answer 1

Answer:

The final temperature is closer to 0 degrees.

Explanation:

Initially we have to use the following formula of heat transfer. Taking into consideration 0,114 cal/g °C as specific heat capacity of the Iron

$0 = (t_{f}-t_{0})*C_{Fe}*M_{Fe} + (t_{f}-t_{0})*C_{H{2O} }*M_{H{2O} \\\\t_{f} = final.temperature\\t_{0} = initial.temperature\\\\C_{Fe} = 0,114 cal/g Celsius\\C_{H2O} = 1 cal/g Celsius\\\\\\M_{H{2O}} = Mass.water\\M_{Fe} = Mass.iron$

By replacing the formula above we have:

$0 = (t_{f}-100 C)*0.114 cal/gC*2kg + (t_{f}-0C)*1 cal/gC }*2kg \\t_{f} = 10.23 Celsius$

Which makes closer of 0 degrees.