Calculate the amount of heat is required to convert 10.0 g of water at 60.0 °C to steam at 120.0 °C. Which of the answers below shows the best estimates of the energy of each step in the process? (Specific heat of water = 4.184 L; Specific heat of steam = 2.010 L; AHvap = 2300 L; Boiling point = 100°C) OA. Energy to ñeat the water = 1700 J Energy to boil the water = 23000 J Energy to heat the steam = 400 J O B. Energy to heat the water = 4.2 J Energy to boil the water = 2300 J Energy to heat the steam = 2.0 J OC. Energy to heat the water = 2500 J Energy to boil the water = 2,300,000 J Energy to heat the steam = 240 J OD. Energy to heat the water = 42 J Energy to boil the water = 230,000 J Energy to heat the steam = 400 J %3D
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.
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