3. A student added calcium to water and measured the increase in temperature to determine AH for the redox reaction: Ca(s) + H₂O(l) → Ca(OH)₂ (aq) + H₂(g). When 0.6418 g Ca was added to 200.0 mL of distilled water in a styrofoam cup, the change in temperature was +8.4°C The density of the water was 1.00 g/mL. a. Which element is being oxidized in this reaction? Which is reduced? b. Calculate the Joules of energy absorbed by the calorimeter, given that Ccal = 20. J/°C. Calculate the Joules of energy absorbed by the solution, given that Ssoln = 4.184 J/g°C. [Note that msoln is the combined weight of water and calcium dissolved into water] d. Calculate the Joules of energy released by the reaction. C.
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.
![3. A student added calcium to water and measured the increase in temperature to determine AH
for the redox reaction: Ca(s) + H₂O(l) → Ca(OH)₂(aq) + H₂(g). When 0.6418 g Ca was
added to 200.0 mL of distilled water in a styrofoam cup, the change in temperature was +8.4°C.
The density of the water was 1.00 g/mL.
a. Which element is being oxidized in this reaction? Which is reduced?
b.
Calculate the Joules of energy absorbed by the calorimeter, given that Ccal = 20. J/°C.
C. Calculate the Joules of energy absorbed by the solution, given that Ssoln = 4.184 J/g°C.
[Note that msoln is the combined weight of water and calcium dissolved into water]
d. Calculate the Joules of energy released by the reaction.
Calculate the enthalpy of reaction, per gram of calcium.
f. Calculate the enthalpy of reaction, per mole of calcium.
e.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa86b2d75-dc89-44ee-816d-e64b811f53cb%2F9006fae3-7218-49a1-ac23-1b6019624768%2Fdyt4od_processed.png&w=3840&q=75)
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