a. Calculate the enthalpy of reaction for: 2 CO(g) + O2(g) → 2 CO2(g) b. If 18.5 grams of carbon dioxide are produced, what is the change in energy in 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.
![### Calculating the Enthalpy of Reaction
**a. Calculate the enthalpy of reaction for:**
\[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]
**b. If 18.5 grams of carbon dioxide are produced, what is the change in energy in kJ?**
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**Explanation:**
To solve part (a), you will need the standard enthalpies of formation for the reactants and products involved in the reaction. The enthalpy change for the reaction \(\Delta H_{reaction}\) can be calculated using Hess's Law:
\[ \Delta H_{reaction} = \Sigma \Delta H_f \text{(products)} - \Sigma \Delta H_f \text{(reactants)} \]
For part (b), use the enthalpy change per mole from part (a) to calculate the energy change for 18.5 grams of \(\text{CO}_2\). First, convert the mass of \(\text{CO}_2\) to moles:
\[ \text{Molar Mass of } \text{CO}_2 = 44.01 \text{ g/mol} \]
\[ \text{Moles of } \text{CO}_2 = \frac{18.5 \text{ g}}{44.01 \text{ g/mol}} \]
Then, multiply the moles by the enthalpy change per mole obtained in part (a) to find the total energy change in kJ.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F26d9d132-de79-44b4-9982-9bb4e4e01868%2Fb9995966-cc41-4f6b-ac5d-39854826bc04%2Fl1jtd78.jpeg&w=3840&q=75)
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