Junisa Jusu (J. Grate)
Jun 27
Defined the following with an example of two balanced chemical equation where possible 1 Entropy 3 Enthalpy 4 Standard heat of formation? ?
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ChatGPT
Jun 27
1. Entropy: Entropy is a measure of the disorder or randomness of a system. It is denoted by the symbol S.
Example of a balanced chemical equation involving entropy:
2H2(g) + O2(g) -> 2H2O(g) + energy
3. Enthalpy: Enthalpy is a measure of the total energy of a system. It is denoted by the symbol H.
Example of a balanced chemical equation involving enthalpy:
2C(s) + 2H2(g) -> C2H4(g)
4. Standard heat of formation: The standard heat of formation is the change in enthalpy that occurs when one mole of a compound is formed from its elements in their standard states. It is denoted by the symbol ΔHf°.
Example of a balanced chemical equation involving standard heat of formation:
2H2(g) + O2(g) -> 2H2O(g) ΔHf° = -483.6 kJ/mol
Example of a balanced chemical equation involving entropy:
2H2(g) + O2(g) -> 2H2O(g) + energy
3. Enthalpy: Enthalpy is a measure of the total energy of a system. It is denoted by the symbol H.
Example of a balanced chemical equation involving enthalpy:
2C(s) + 2H2(g) -> C2H4(g)
4. Standard heat of formation: The standard heat of formation is the change in enthalpy that occurs when one mole of a compound is formed from its elements in their standard states. It is denoted by the symbol ΔHf°.
Example of a balanced chemical equation involving standard heat of formation:
2H2(g) + O2(g) -> 2H2O(g) ΔHf° = -483.6 kJ/mol
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Google Gemini AI
Jun 27
1. Entropy
Entropy is a measure of the disorder or randomness of a system. The higher the entropy, the more disordered the system.
Example:
- Melting of ice: Ice is a solid with a low entropy, while water is a liquid with a higher entropy. When ice melts, the entropy of the system increases.
2. Enthalpy
Enthalpy is a thermodynamic property that measures the total energy of a system. It is defined as the sum of the internal energy of the system and the product of the pressure and volume.
Example:
- Combustion of methane: Methane is a gas with a high enthalpy, while carbon dioxide and water are gases with lower enthalpies. When methane burns, the enthalpy of the system decreases.
3. Standard Heat of Formation
The standard heat of formation is the enthalpy change that occurs when one mole of a compound is formed from its constituent elements in their standard states (25°C and 1 atm).
Example:
- Formation of water: Hydrogen and oxygen gases react to form water with a standard heat of formation of -285.8 kJ/mol.
Entropy is a measure of the disorder or randomness of a system. The higher the entropy, the more disordered the system.
Example:
- Melting of ice: Ice is a solid with a low entropy, while water is a liquid with a higher entropy. When ice melts, the entropy of the system increases.
2. Enthalpy
Enthalpy is a thermodynamic property that measures the total energy of a system. It is defined as the sum of the internal energy of the system and the product of the pressure and volume.
Example:
- Combustion of methane: Methane is a gas with a high enthalpy, while carbon dioxide and water are gases with lower enthalpies. When methane burns, the enthalpy of the system decreases.
3. Standard Heat of Formation
The standard heat of formation is the enthalpy change that occurs when one mole of a compound is formed from its constituent elements in their standard states (25°C and 1 atm).
Example:
- Formation of water: Hydrogen and oxygen gases react to form water with a standard heat of formation of -285.8 kJ/mol.
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