If the heat of combustion for a specific compound is -1120.0 kJ/mol and its molar mass is 98.67 g/mol, how many grams of this compound must you burn to release 872.10 kJ of heat? mass: g
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.
![**Transcription for Educational Website:**
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**Heat of Combustion Calculation**
In this exercise, you are given the following problem:
"If the heat of combustion for a specific compound is –1120.0 kJ/mol and its molar mass is 98.67 g/mol, how many grams of this compound must you burn to release 872.10 kJ of heat?"
**Calculation Requirements:**
- **Heat of Combustion**: –1120.0 kJ/mol
- **Molar Mass**: 98.67 g/mol
- **Target Energy Release**: 872.10 kJ
**Solution Steps:**
1. **Determine the Number of Moles Needed**:
- Use the equation:
\[
\text{moles} = \frac{\text{Target Energy Release}}{\text{Heat of Combustion}}
\]
2. **Calculate the Mass**:
- Multiply the number of moles by the molar mass to find the mass required.
**Mass Required**:
\[ \text{mass} = \]
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*Please input the calculations in the box provided to find the precise mass in grams.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F76884ef0-0050-4a4d-a83f-5c6d84fc3fcd%2Ffaf0d1ca-e06e-485e-8b2f-2995da3eaca6%2Fjkp6wu_processed.jpeg&w=3840&q=75)
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