f a 125 g sample of iron is heated to 250.0oC and then placed in 500.0 g of water at 25.0 oC in an insulated container, what will the final temperature of the water and iron be? Assume that all of the heat transfers from the iron to the water without loss to the surroundings. ( qH2O = -q Fe ) ( Like the question at the start of lecture 5.2) cs (Fe) = 0.450 J/goC cp (H2O) = 4.18 J/goC
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
If a 125 g sample of iron is heated to 250.0oC and then placed in 500.0 g of water at 25.0 oC in an insulated container, what will the final temperature of the water and iron be? Assume that all of the heat transfers from the iron to the water without loss to the surroundings. ( qH2O = -q Fe )
( Like the question at the start of lecture 5.2)
cs (Fe) = 0.450 J/goC cp (H2O) = 4.18 J/goC
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
