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1. Choose the CORRECT statement:
Exothermic reactions are always spontaneous
Free energy is independent of temperature.
A reaction which exhibits a negative value of D S cannot be spontaneous.
At constant P and T, a decrease in free energy insures an increase in the entropy of the system.
None of the above statements are true.

2. For the phase change of liquid to solid, DS is:
0
positive
negative
positive at high temperature
none of the above

3. 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 DSsurroundings.
0
69.0 kJ/mol
71.9 J/K mol
61.0 kJ/mol
-71.9 J/K mol

4. Which of these statements is false?
For a spontaneous reaction DG is negative
Independent of T, a reaction must be spontaneous if DH = 0 and DS is positive
A spontaneous reaction is always fast
A spontaneous reaction occurs without outside intervention
None of the above is false

5. A change of state occurs within a system and produces 64.0 kB of heat which is transferred to the surrounding at a constant pressure and a constant temperature of 300K. For this process DSsurroundings is:
64.0 kJ
-64.0 kJ
-213 J/K
213 J/K
none of these

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