Suppose 1.00 mol superheated ice melts to liquid water at 25°c. assume the specific heats of ice and liquid water have the same value and are independent of temperature. the enthalpy change for the melting of ice at 0°c is 6007 j mol21. calculate dh, dssys, and dg for this process.

Enthalpy change is 6007 J

Entropy change is

Gibb's free energy change is 0 J.

Explanation:

From the given,

The enthalpy change for the melting of ice =

Temperature =

Let's convert the temperature centigrade into Kelvin.

Number of moles of ice = 1.00 mol

Enthalpy change of 1.00 mol temperature

Therefore, Enthalpy change () for the melting of 1.00 mole of ice at temperature is 6007 J.

Entropy change for the melting of 1.00 mole of ice at :

Therefore, Entropy change()  for the melting of 1.00 mole of ice at temperature is .

The Gibb's free energy change is expressed by the following formula.

Therefore, Gibb's free enrgy change () for the melting of 1.00 mole of ice at temperature is

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