A.) If 1.22 KJ of heat is added to 50 grams of the water at 25.0 oC, What is the final temperature of the water? (Specific heat of water is 4.184 J/goC) B.) A 20.0 gram piece of hot iron at 225oC is placed in a 51.0 gram sample of water. No heat escapes to the surroundings. The water and iron equilibrate at 45oC. How much did the temperature of the water increase? C.) What is the specific heat of nickel if the temperature of a 32.2 grams sample of nickel is increased by 3.5oC when 50.0 Joules of heat is added?
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.
A.) If 1.22 KJ of heat is added to 50 grams of the water at 25.0 oC, What is the final temperature of the water? (Specific heat of water is 4.184 J/goC)
B.) A 20.0 gram piece of hot iron at 225oC is placed in a 51.0 gram sample of water. No heat escapes to the surroundings. The water and iron equilibrate at 45oC. How much did the temperature of the water increase?
C.) What is the specific heat of nickel if the temperature of a 32.2 grams sample of nickel is increased by 3.5oC when 50.0 Joules of heat is added?
Trending now
This is a popular solution!
Step by step
Solved in 5 steps
