A student heats a 12.65 g sample of iron for 5 minutes until it reaches a constant temperature 100°C. They immediately add it to a beaker of water with an initial temperature of 21.3°C. After 2 minutes, the temperature of the water in the beaker remains constant at 23.5°C. How much energy did the sample of iron lose? (Note: the mass of water in the beaker is 50.0 gram)

Explanation:

A student heats a 12.65 g sample of iron for 5 minutes until it reaches a constant temperature 100°C. They immediately add it to a beaker of water with an initial temperature of 21.3°C. After 2 minutes, the temperature of the water in the beaker remains constant at 23.5°C. How much energy did the sample of iron lose? (Note: the mass of water in the beaker is 50.0 gram)

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.

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.