Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas: Al (s) + 3 HCI (1) → AICI3 (aq) + H2 (g) When 2.683 g of Al is combined with enough hydrochloric acid to make 200.0 mL of solution in a coffee-cup calorimeter, all af the Al reacts, raising the temperature of the solution from 25 °C to 29.2 °C. Find the AHrxn in kJ for the reaction as written. (Assume that the specific heat capacity of the solution is 4.184 J/g °C and the density is 1.00 g/mL.)
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.
![**Reaction of Aluminum with Hydrochloric Acid**
Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas:
\[ \text{Al (s) + 3 HCl (l) } \rightarrow \text{ AlCl}_3 \text{ (aq) + H}_2 \text{ (g)} \]
When 2.683 g of Al is combined with enough hydrochloric acid to make 200.0 mL of solution in a coffee-cup calorimeter, all of the Al reacts, raising the temperature of the solution from 25 °C to 29.2 °C. Find the \(\Delta H_{\text{rxn}}\) in kJ for the reaction as written. (Assume that the specific heat capacity of the solution is 4.184 J/g °C and the density is 1.00 g/mL.)
**Your Answer:**
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In this setup, students are tasked with calculating the enthalpy change (\(\Delta H_{\text{rxn}}\)) of a reaction involving aluminum and hydrochloric acid, using calorimetric data. The specific heat capacity and density of the solution are provided to aid in the calculation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7269c65d-b7b5-4fbf-8945-da94b0914ae2%2F2e5d4477-9f88-46c6-b0e0-258e78108bd1%2Fj3ymhz_processed.jpeg&w=3840&q=75)
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