Using the following data calculate Delta Sfus and Delta Svap for K in J/mol-k

Tm(K) = 336,
Delta H Fus(kJ/mol) = 2.33,
Tb (K) = 1033,
Delta H vap (kJ/mol) = 77.1

For Delta S fus i'm supposed to use 336 K the Tm value and for Delta S vap i'm supposed to use 1033 K the Tb value is that correct..?

Something that worries me is that the problem even uses "Tm" and "Tb" .. am i supposed to do conversions?

Oh dear, it seems you're in need of some clownish wisdom for your thermodynamic calculations!

Well, to find Delta Sfus (the entropy change during fusion) and Delta Svap (the entropy change during vaporization) for K, you're on the right track!

For Delta Sfus, you need to use the Tm value of 336 K. Now, we know that entropy change during fusion can be calculated using the formula Delta S = (Delta Hfus / T), where Delta Hfus is the enthalpy of fusion and T is the temperature. Since Delta Hfus is given as 2.33 kJ/mol and T is 336 K, just plug in the values and voila! You'll get the change in entropy during fusion for K.

On the other hand, for Delta Svap (the entropy change during vaporization), you indeed need to use the Tb value of 1033 K. Similar to Delta Sfus, you can use the formula Delta S = (Delta Hvap / T), where Delta Hvap is the enthalpy of vaporization. With the given value of Delta Hvap as 77.1 kJ/mol and T as 1033 K, go ahead and calculate Delta Svap.

Remember, clowns like me are here to entertain and bring a smile to your face, so don't let these calculations make you frown! Enjoy the process and let me know if you need further assistance!

Yes, that is correct. To calculate Delta Sfus (change in entropy for fusion) and Delta Svap (change in entropy for vaporization), you should use the respective melting point (Tm) and boiling point (Tb) temperatures.

For Delta Sfus, you would use Tm = 336 K.

For Delta Svap, you would use Tb = 1033 K.

Yes, that is correct. To calculate ΔSfus (change in entropy of fusion) and ΔSvap (change in entropy of vaporization), you need to use the melting point temperature (Tm) and the boiling point temperature (Tb) respectively.

First, let's convert the given values of ΔHfus (enthalpy of fusion) and ΔHvap (enthalpy of vaporization) from kJ/mol to J/mol:
ΔHfus = 2.33 kJ/mol = 2330 J/mol
ΔHvap = 77.1 kJ/mol = 77100 J/mol

To calculate ΔSfus, you can use the equation:
ΔSfus = ΔHfus / Tm

Plugging in the values:
ΔSfus = 2330 J/mol / 336 K
ΔSfus ≈ 6.933 J/mol-K

To calculate ΔSvap, you can use the equation:
ΔSvap = ΔHvap / Tb

Plugging in the values:
ΔSvap = 77100 J/mol / 1033 K
ΔSvap ≈ 74.64 J/mol-K

So, the values for ΔSfus and ΔSvap are approximately 6.933 J/mol-K and 74.64 J/mol-K respectively.

I assume Tm stands for the melting point temperature while Tb stands for the boiling point temperature.

dG = dH - TdS
At the melting point the system is in equilibrium between the solid and the liquid; at the boiling point the system is in equilibrium between the liquid and vapor.
0 = 2330 - TdS
Plug in Tm and solve for dS fusion

0 = 77100 - TdS
Plug in Tb and solve for dS vaporization.