Question

The reaction of MnO4 with oxalic acid (H2C204) in acidic solution, yielding Mn2+ and CO2 gas, is widely used to determine the concentration of permanganate solutions. a. Write a balanced equation for the reaction. b. Show that the reaction goes to completion by calculating the values of AGº and K at 25 °C. Most values for AG°f are in the back of your textbook. AG°f of H2C2O4(aq) is -674.0 kJ/mol. If your calculator will not give you an actual value of K, just use the exponential expression (e###). Again, provide some reasoning for what you are doing.

Answer 1

Q. a) Mnog +8Ht+ se - Mn2t + 4H2O X2 (2092 - → 2.02 +2e x 5 2 uno +56202 + 16Ht s 2 Mn2r + 10 202 + 8 H₂0 by 46 = 200;4) +10 36if (63) +8862CH2O) – 20694 (M104") -5464 (202) Given su plas) = - 394.39 kJ/mot , AG (h): - 237-14 kg/mo) , AGg (mnog) = -449.4 4 kg/mol AGf (1209 1 = -674-0 kylmol , AGf (Mn2+) = -228.0 kJ/mot -2028.22 kJ/mol i OG

we know T=256- 724४ Again AG == RT ln K =>(-2 2028-22 x103 g mois 18.3 1 8.314 Jik'.mo )x(298k) x luk -) enk = 818.63 818.63 e K = = 2225.27 The ralece of the equilibrium constant is very high implying that the equilibrium mostly lies in the product side. Hence the reaction go to completion.