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1. Which of the following favors a negative DG?
increasing energy and increasing entropy
lowering energy and increasing entropy
increasing energy and decreasing entropy
lowering energy and decreasing entropy
none of the above

2. Which statement is FALSE?
DS increases as pressure decreases
for an ideal gas, enthalpy is not pressure-dependent
the lowest value of free energy occurs at equilibrium
DS increases as volume increases
all statements are true

3. Choose the correct statement.
Exothermic reactions are always spontaneous
High temperature ensures a spontaneous reaction
Free energy is independent of temperature
A reaction with negative DS cannot be spontaneous
none of the above

4. 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

5. 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

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