Calculate the standard reaction enthalpies, the standard reaction entropy and the standard reaction Gibbs at 298 K of a. Zn(s) + Cu²+(aq) → Zn2+(aq) + Cu(s) b. C12H22O11(S) + 12 O2(g) → 12 CO2(g) +11 H2O(1)

Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.

Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.

Predict whether each reaction is reactant-favored or product-favored at 298 K and 1 bar, and calculate the minimum work that would have to be done to force it to occur, or the maximum work that could be done by the reaction. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)

The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).

Σ II For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N,(g) + 3 H, (g) = 2 NH, (g) the standard change in Gibbs free energy is AG° = –32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.450 atm, PH, = 0.250 atm, and PNH = 0.650 atm? kJ/mol = 9V 50:8 11/8 PrtScr Insert Delete F10 F11 F12 F7 F4 KA & Backspac 24 % 60 H. B.

Chemistry Using the information in the data section, calculate the standard reaction ent and standard reaction Gibbs energy for the n2(g)+3h2(g) → 2nh3(g) reaction.

An aqueous solution of 49.60 ml of 0.370mol L-1 NaCN is added to 49.60 ml of 0.370 mol L-1 Zn(NO3)2 (aq) at 25°C. Determine the concentration (in mol L-1) of Zn(CN)42- in the solution once it reaches thermodynamic equilibrium at 25°C. Kf (Zn(CN)42-) = 2.1 X 1019

The equilibrium constant of the reaction 2 C3H6(g) ⇋ C2H4(g) + C4H8(g) is found to fit the expression ln K = A + B/T + C/T2 between 300 K and 600 K, with A = −1.04, B = −1088 K, and C = 1.51 × 105 K2. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K.