Final answer:
The entropy change for the conversion of 1g of ice to H₂O at 273K and 1 atm pressure is approximately 0.001 J/K.
Step-by-step explanation:
The entropy change for the conversion of 1g of ice to H₂O at 273K and 1 atm pressure can be calculated using the formula:
ΔS = Q/T
Where Q is the heat absorbed during the conversion and T is the temperature in Kelvin. The enthalpy of fusion of ice is given as 6.025 kJ/mol. To calculate the amount of heat absorbed, we can use the equation:
Q = n * ΔH
Where n is the number of moles and ΔH is the enthalpy of fusion. Since we are given 1g of ice, we need to convert it to moles by using the molar mass of water. The molar mass of water is approximately 18.02 g/mol. Therefore, 1g of ice is equal to 1/18.02 mol. Plugging in these values, we can calculate the amount of heat absorbed:
Q = (1/18.02 mol) * 6.025 kJ/mol = 0.334 kJ
Now, we can plug this value of Q into the entropy formula:
ΔS = 0.334 kJ / 273 K = 0.001 J/K