When 0.361 g of sodium metal is added to an excess of hydrochloric acid, 3750 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCl(aq) → 2 NaCl(aq) + H,(g) Enthalpy of reaction: kJ
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.
![**Determining the Enthalpy of Reaction**
In this problem, we are asked to find the enthalpy change of a chemical reaction where sodium metal is added to an excess of hydrochloric acid. Here's the scenario:
- A sample of 0.361 g of sodium metal is added to hydrochloric acid.
- This reaction releases 3750 J of heat.
The chemical equation for this reaction is:
\[ \text{2 Na(s) + 2 HCl(aq) } \rightarrow \text{2 NaCl(aq) + H}_2\text{(g)} \]
The task is to calculate the enthalpy of the reaction as written, reported in kilojoules (kJ).
**Enthalpy of reaction: \_\_\_ kJ**
To complete this calculation:
1. Convert the heat produced (3750 J) to kilojoules by dividing by 1000.
2. Calculate the enthalpy change per mole of sodium using stoichiometry from the balanced equation.
Make sure to express your final answer in kilojoules (kJ).
Note: This exercise is useful for understanding reaction energetics and calorimetry in chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd15a2d56-c982-4a4b-8f12-312dac46f35d%2F99d08882-b4d0-4e7f-a0ee-1220ead73aa8%2F6fem7eu_processed.jpeg&w=3840&q=75)
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