A calorimeter contains 130 g water. The calorimeter and the water inside are both at 26 °C. A piece of metal weighing 35 g was heated to 90 °C and then put into the water inside the calorimeter. The equilibrium temperature was determined to be 35 °C. Assuming no heat is lost to the environment, calculate the specific heat of the metal. Calorimeter constant: 120 J°c-1 Specific heat of water: 4.184 J°C1g1 O A. 3.85 J°C'g1 O B. 2.18 J°C-'g*1 Oc 3.10 J°C-'g"1 O D. 2.54 J°C'g1 O E. 2.67 J°C-'g"1
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.
Step by step
Solved in 2 steps
