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Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹?
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Calculate the entropy change during the melting of one mole of ice int...
Entropy Change Calculation
To calculate the entropy change during the melting of ice at 0 °C and 1 atm, we can use the formula:
ΔS = ΔH/T
Where:
- ΔS = Change in entropy (J/K·mol)
- ΔH = Enthalpy of fusion (J/mol)
- T = Temperature (K)
Given Values
- Enthalpy of fusion (ΔH) = 6008 J/mol
- Temperature (T) = 0 °C = 273.15 K (converted to Kelvin)
Calculating Entropy Change
1. Convert Temperature to Kelvin:
- T = 0 °C + 273.15 = 273.15 K
2. Apply the Entropy Change Formula:
- ΔS = ΔH/T
- ΔS = 6008 J/mol / 273.15 K
3. Perform the Calculation:
- ΔS ≈ 22.0 J/K·mol
Significance of the Result
- The positive value of ΔS indicates an increase in disorder as ice melts into water.
- This is consistent with thermodynamic principles, where melting involves a transition from a structured solid to a less ordered liquid state.
Conclusion
- The entropy change during the melting of one mole of ice at 0 °C and 1 atm is approximately 22.0 J/K·mol.
- This change highlights the thermodynamic favorability of the melting process, reinforcing the concept of increased randomness in the system.
To calculate the entropy change during the melting of ice at 0 °C and 1 atm, we can use the formula:
ΔS = ΔH/T
Where:
- ΔS = Change in entropy (J/K·mol)
- ΔH = Enthalpy of fusion (J/mol)
- T = Temperature (K)
Given Values
- Enthalpy of fusion (ΔH) = 6008 J/mol
- Temperature (T) = 0 °C = 273.15 K (converted to Kelvin)
Calculating Entropy Change
1. Convert Temperature to Kelvin:
- T = 0 °C + 273.15 = 273.15 K
2. Apply the Entropy Change Formula:
- ΔS = ΔH/T
- ΔS = 6008 J/mol / 273.15 K
3. Perform the Calculation:
- ΔS ≈ 22.0 J/K·mol
Significance of the Result
- The positive value of ΔS indicates an increase in disorder as ice melts into water.
- This is consistent with thermodynamic principles, where melting involves a transition from a structured solid to a less ordered liquid state.
Conclusion
- The entropy change during the melting of one mole of ice at 0 °C and 1 atm is approximately 22.0 J/K·mol.
- This change highlights the thermodynamic favorability of the melting process, reinforcing the concept of increased randomness in the system.
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Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹?
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Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹?.
Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Calculate the entropy change during the melting of one mole of ice into water at 0 degree Celsius and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol‐¹?.
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