Which of the following is a reaction rate?   ∆mol/∆L   ∆mol/∆s   ∆M/∆V   ∆mol/∆g

At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 10? Is this a thermodynamically-favorable reaction? 2. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 100? Is this a thermodynamically-favorable reaction? 3. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 0.1? Is this a thermodynamically-favorable reaction?               4. At 25 ̊C, what is the free energy (∆G ̊) of a reaction with Keq = 0.01? Is this a thermodynamically-favorable reaction? 5. What do you notice about the sign of ∆G ̊ and the magnitude of Keq? 6. What is the change in ∆G ̊ when Keq increases by a factor of 10? 100? Write 1-2 sentences to describe this relationship.

Consider the reaction: ICl(g) + Cl₂(g) → ICl₃(s). The ∆G(f)° of ICl(g) is -5.5 kJ/mol and the ∆G(f)° of ICl₃(s) is -22.59 kJ/mol What is the ∆G° of the reaction, in kJ/mol?

For certain chemical reaction ∆H = 15 kJ/mol and ∆S = 51 J mol-1 K-1, What is ∆G (in kJ/mol)  for the reaction when T = a 0o ? A) 1.07 B) -1007 C) 0.107 D) 1007  E) -1.07

Consider the following reaction at equilibrium: 2NO₂(g) ⇌ N₂O₄(g) The ∆H° for this reaction is < 0. If the volume of the container is decreased by ½ while the temperature is kept constant, how will K(eq) change?

11. This reaction must have a ∆G>0 at SATP:   2O3(g)→3O2(g)   C(s)+O2(g)→CO2(g)   2K(s)+F2(g)→KF2(s)   2Fe2O3(s)→4Fe(s)+3O2(g)

What is S° for B in the reaction 3 A → 2 B if ∆S°(rxn) =-227.8 J/mol ･ K? [S° (A) = (205.0 J/mol ･K)]

(a)        N2(g)               +          O2(g)                           2NO (g)            ∆H298 = + 180 kJ mol-1    From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:   Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalyst