Question:
What is the entropy change (in JK–1mol–1) when one mole of ice is converted into water at 0ºC?(The enthalpy change for the conversion of ice to liquid water is 6.0 KJ mol–1 at 0ºC)
What is the entropy change (in JK–1mol–1) when one mole of ice is converted into water at 0ºC?(The enthalpy change for the conversion of ice to liquid water is 6.0 KJ mol–1 at 0ºC)
Updated On: Jul 26, 2024
20.13
2.013
2.198
21.98
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The Correct Option is D
Solution and Explanation
you can use the equation:
\(\Delta S=\frac{\Delta H}{T}\)
Given:
Enthalpy change (ΔH) = 6.0 kJ/mol = 6.0kJ/mol×1000J/kJ = 6000J/mol
Temperature (T) = 0°C = 273.15 K
Now, plug the values into the equation:
ΔS = \(\frac{6000\,J/mol}{273.15\,K}\)
ΔS ≈ 21.98 J/K/mol
So, the correct answer is (D): 21.98 J/K/mol
\(\Delta S=\frac{\Delta H}{T}\)
Given:
Enthalpy change (ΔH) = 6.0 kJ/mol = 6.0kJ/mol×1000J/kJ = 6000J/mol
Temperature (T) = 0°C = 273.15 K
Now, plug the values into the equation:
ΔS = \(\frac{6000\,J/mol}{273.15\,K}\)
ΔS ≈ 21.98 J/K/mol
So, the correct answer is (D): 21.98 J/K/mol
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