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.

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:

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.