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The change in the entropy for the fusion of 1 mole of ice is:
(Melting point of ice = 273 K, molar enthalpy of fusion of ice = 6.0 KJ mol–1):
- a)11.73 JK–1mol–1
- b)18.84 JK–1mol–1
- c)21.97 JK–1mol–1
- d)24.47 JK–1mol–1
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
The change in the entropy for the fusion of 1 mole of ice is:(Melting ...
Change in Entropy 
= 
(Enthaply of fusion) /T (Temperature)
= (Enthaply of fusion) /T (Temperature)= 60*103 / 273
= 21.97 J/K/mol
Most Upvoted Answer
The change in the entropy for the fusion of 1 mole of ice is:(Melting ...
Entropy Change for the Fusion of Ice
The entropy change for the fusion of 1 mole of ice can be calculated using the equation:
ΔS = ΔH / T
where ΔS is the change in entropy, ΔH is the molar enthalpy of fusion, and T is the temperature in Kelvin.
Gathering the Given Information
From the question, we are given the following information:
- Melting point of ice = 273 K
- Molar enthalpy of fusion of ice = 6.0 kJ mol^-1
Converting Units
To use the given information in the entropy change equation, we need to convert the molar enthalpy of fusion from kJ to J.
Given: 1 kJ = 1000 J
Therefore, the molar enthalpy of fusion of ice is:
ΔH = 6.0 kJ mol^-1 = 6.0 x 1000 J mol^-1 = 6000 J mol^-1
Calculating the Entropy Change
Now that we have the values for ΔH and T, we can substitute them into the entropy change equation:
ΔS = ΔH / T
ΔS = 6000 J mol^-1 / 273 K
Calculating the value:
ΔS ≈ 21.98 J K^-1 mol^-1
Final Answer
Rounding to the appropriate number of significant figures, the change in entropy for the fusion of 1 mole of ice is approximately 21.97 J K^-1 mol^-1.
Therefore, the correct answer is option 'C': 21.97 JK1mol1.
The entropy change for the fusion of 1 mole of ice can be calculated using the equation:
ΔS = ΔH / T
where ΔS is the change in entropy, ΔH is the molar enthalpy of fusion, and T is the temperature in Kelvin.
Gathering the Given Information
From the question, we are given the following information:
- Melting point of ice = 273 K
- Molar enthalpy of fusion of ice = 6.0 kJ mol^-1
Converting Units
To use the given information in the entropy change equation, we need to convert the molar enthalpy of fusion from kJ to J.
Given: 1 kJ = 1000 J
Therefore, the molar enthalpy of fusion of ice is:
ΔH = 6.0 kJ mol^-1 = 6.0 x 1000 J mol^-1 = 6000 J mol^-1
Calculating the Entropy Change
Now that we have the values for ΔH and T, we can substitute them into the entropy change equation:
ΔS = ΔH / T
ΔS = 6000 J mol^-1 / 273 K
Calculating the value:
ΔS ≈ 21.98 J K^-1 mol^-1
Final Answer
Rounding to the appropriate number of significant figures, the change in entropy for the fusion of 1 mole of ice is approximately 21.97 J K^-1 mol^-1.
Therefore, the correct answer is option 'C': 21.97 JK1mol1.
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Community Answer
The change in the entropy for the fusion of 1 mole of ice is:(Melting ...
∆S=∆H/T for reversible phase transition .
∆S=6000/273
∆S=6000/273
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The change in the entropy for the fusion of 1 mole of ice is:(Melting point of ice = 273 K, molar enthalpy of fusion of ice = 6.0 KJ mol–1):a)11.73 JK–1mol–1b)18.84 JK–1mol–1c)21.97 JK–1mol–1d)24.47 JK–1mol–1Correct answer is option 'C'. Can you explain this answer?
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