Thermochemical equations Thermochemical equations are chemical equations that clearly show the relationship between mass of products and reactants and enthalpy changes. For example CH4 (g) + 202 (g) → CO2 (g) + 2H2O (1) AH = - 890.4 kJ moles of CH4 = - 890.4 kJ moles of O2 = - 890.4 kJ moles of CO2 = - 890.4 kJ moles of H20 = - 890.4 kJ - 890.4 kJ mol - 890.4 kJ - 890.4 kJ - 890.4 kJ mol mol mol Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen. Determine the heat produced in the above reaction when 1.6 grams of oxygen is burned in excess methane.
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.
Please help me complete question 1 and 2
![**Thermochemical Equations**
Thermochemical equations are chemical equations that clearly show the relationship between the mass of products and reactants and enthalpy changes. For example:
\[ \text{CH}_4 (g) + 2\text{O}_2 (g) \rightarrow \text{CO}_2 (g) + 2\text{H}_2\text{O} (l) \hspace{20pt} \Delta H = -890.4 \, \text{kJ} \]
- ___ moles of \(\text{CH}_4\) = -890.4 kJ
- ___ moles of \(\text{O}_2\) = -890.4 kJ
- ___ moles of \(\text{CO}_2\) = -890.4 kJ
- ___ moles of \(\text{H}_2\text{O}\) = -890.4 kJ
\[
-\frac{890.4 \, \text{kJ}}{\text{mol}} \hspace{70pt} -\frac{890.4 \, \text{kJ}}{\text{mol}} \hspace{70pt} -\frac{890.4 \, \text{kJ}}{\text{mol}} \hspace{80pt} -\frac{890.4 \, \text{kJ}}{\text{mol}}
\]
**Questions:**
i. Determine the heat produced in the above reaction when 1.6 grams of methane is burned in excess oxygen.
ii. Determine the heat produced in the above reaction when 1.6 grams of oxygen is burned in excess methane.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F921f6546-af39-43f1-aaa9-36572b00cf90%2F6f4e3b9f-1fc2-4ac9-9938-634f5dd38cac%2F5oljva_processed.jpeg&w=3840&q=75)
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