Question

A piece of iron with a mass of 56.2 grams is heated and placed into a calorimeter containing 93.64 grams of water at 7.0 degrees Celsius. The final temperature of the water and the iron is 90.5 degrees Celsius. Assuming no heat is lost to the surroundings, how much heat (in Joules) does the iron release? Round your answer to the nearest 0.1 Joules.

Answer 1

`Q_(iron) = -32730.083\,J`

Step-by-step explanation:

By the First Law of Thermodynamics, the piece of iron and water reach thermal equilibrium when both have the same temperature. The heat released by the piece of iron is received by the water. That is to say:

`Q_(iron) = -Q_(w)`

`Q_(iron) = (93.64\,g)\cdot \left(4.186\,(J)/(kg\cdot ^(\textdegree)C) \right)\cdot (7\,^(\textdegree)C-90.5\,^(\textdegree)C)`

`Q_(iron) = -32730.083\,J`