Using the following values & equations, Cs,ice 2.09 J/g°C, Cs,water (1) 4.184 J/g°C, AHvap, H20 +40.7 kJ/mol, q = nΔΗfus, q = nΔΗvap, q=mx Cs x AT Calculate the amount of energy (in kJ) that it would take to increase the temperature of 2.0 mol of ice from -75.0 °C to water vapor at a temperature of 150 °C. Input your answer without units! (But make sure the answer you input is in kJ) Cs,water (g)= 2.01 J/gºC, AHfus, H20 +6.02 kJ/mol,
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.
Well, we have to calculate the energy in each step and added them up to get the overall energy required.
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