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1. For the dissociation reaction of the acid HF: HF<-->H++ F -
DS is observed to be negative. The BEST explanation for this is:

This is the expected result since each HF molecule produces two ions when it dissassociates
Hydration of the ions produces the negative value of DS.
The reation is expected to be exothermic and thus D should be negative.
The reaction is expected to be endothermic and thus D should be negative.
None of these can explain the negative value of DS.

2. The 3rd Law of Thermodynamics States that:
Energy is artificial
Energy can neither be created nor lost
The entropy of the universe is decreasing
The entropy is zero at zero K for a perfect crystal
none of the above

3. A system can achieve the lowest possible free energy by going into:
high pressure
presence of catalyst
equilibrium
completion
none of the above

4. If an endorthermic reaction is spontaneous at 298 K, which of the following must be true for the reaction?
DG is greater than zero
DG is greater than zero
DG and DH are greater than zero
DH and DS are greater than zero
DG, DH, DS are all greater than zero

5. Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686oC). For the process Rb(l)-->Rb(g) at 1 atm and 686oC. Calculate the value of DG.
0
69.0 kJ/mol
71.9 J/K mol
61.0 kJ/mol
-7.97 kJ/mol

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