If a 50.0 gram piece of copper is heated to 100oC and then put into a vessel containing 50.0 grams of water at 11oC. Take the molar heat capacity of copper to be 24.4 ? / ??? ?? and that of water to be 75.3 ? / ??? ?? Molar mass of copper is 63.55 g/mol and the molar mass of water is 18.02 g/mol. 24) How many moles of copper are involved in the above reaction? What will be the final temperature of the water (in oC)? a) 95oC b) 55oC c) 18oC d) 2.0oC Note: I think I understand how to set up the problem, but am lost on the algebra to settle for T-final. My setup: 0.78678 mol Cu * 24.4 J/mol oC * (T final - 100 oC) = -2.7746 mol H2O * 75.3 J/mol oC * (T final - 11 oC) Thanks!
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 50.0 gram piece of copper is heated to 100oC and then put into a vessel containing 50.0 grams of water at 11oC.
Take the molar heat capacity of copper to be 24.4 ? / ??? ?? and that of water to be 75.3 ? / ??? ??
Molar mass of copper is 63.55 g/mol and the molar mass of water is 18.02 g/mol. 24) How many moles of copper are involved in the above reaction?
What will be the final temperature of the water (in oC)?
a) 95oC
b) 55oC
c) 18oC
d) 2.0oC
Note: I think I understand how to set up the problem, but am lost on the algebra to settle for T-final. My setup:
0.78678 mol Cu * 24.4 J/mol oC * (T final - 100 oC) = -2.7746 mol H2O * 75.3 J/mol oC * (T final - 11 oC)
Thanks!
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