What is the standard free energy change and the equilibrium constant for the following reaction at room temperature? Is the reaction spontaneous? Sn(s) + 2Cu2+(aq) ⇋ Sn2+(aq) + 2Cu+(aq)

› Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au³ +(aq) + 3 Ni(s) = 2 Au(s) + 3 Ni² + (aq) AGⓇ = kJ

Calculate the standard free‑energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this table.   2Au3+(aq)+3Ni(s)↽−−⇀2Au(s)+3Ni2+(aq) Δ?∘=   kJ/mol

For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g)        ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)      ?o=−0.403 V   Calculate the H+ concentration in M.

Using the following standard (reduction) potential data:    Br2(aq) + 2 e− → 2 Br−(aq),    1.087 V    2 I−(aq) → I2(s) + 2 e−,    0.535 VCalculate the standard free-energy change (ΔG°) for the following oxidation-reduction reaction. 2 I−(aq) + Br2(aq) → I2(s) + 2 Br−(aq) ?J(b) Calculate the equilibrium constant for this reaction at 298 K.

The oxidation of methanol, as described by the equation below, has a ΔG° value of -937.9 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)

5. The oxidation of ferrous iron (Fe2+) to ferric ion (Fe³+) by molecular oxygen can be described by the following reaction: 4Fe²+ (aq) + O₂(aq) + 4H*(aq) = 4Fe³+ (aq) + 2H₂O(l) (1) Using free energies of formation, calculate the equilibrium constant for this reaction at 25 deg C. (2) For a water in equilibrium with the atmosphere, a pH of 2.0, and a total soluble iron concentration of 1 mg/L, calculate the concentrations of Fe2+(aq) and Fe³+(aq).