1. On the basis of your experience, predict which of the following reactions are spontaneous. 1) NaCl(s)→→ NaCl(/) at 25 °C 2) 2 NaCl(s) → 2 Na(s) + Cl₂(g) 3) CO2(g) → CO2(s) at 25 °C 4) CO2(g) → C(s) + O2(g) 5) H₂O(s)→ H₂O() at 25 °C a) 1, 2, and 3 b) 1, 2, and 4 c) 3 and 5 d) 3 e) 5

Determine whether the following reactions are spontaneous or non-spontaneous. a) N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g), ΔG = -32,960 J b) 2 NH3 (g) ⟶ N2 (g) + 3 H2 (g), ΔG = 32,960 J HINT: The change in free energy (ΔG) for reaction is equal to the difference in free energy between the products (Gproducts) and the reactants (Greactants): ΔG = (Gproducts) - (Greactants) In spontaneous reactions, the free energy of the products (Gproducts) of a reaction is less than the free energy of the reactants (Greactants). When this is the case, will the change in free energy (ΔG) will have a negative value or a positive value?

Does the entropy increase or decrease in these reactions? Why? a) 4 Al + 3 O2 → 2 Al2O3 b) C + 2 Cl2 → CCl4 c) H2O (l) → H2O (g) d) CCl4 → C + 2 Cl2

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ