The permanganate ion is a common oxidizing agent. What is the standard potential of the MnO4–,H+/Mn2+ couple at pH = 6? Report the answer in Volts.
The permanganate ion is a common oxidizing agent. What is the standard potential of the MnO4–,H+/Mn2+...
MnO4- + I− → Mn2+ + I2 in this equation, which is the oxidizing agent reducing agent species that has been reduced species that has been oxidized
5. (20pts) Consider the reaction between oxalate ion and permanganate ion in acidic solution: MnO4 (aq) + C202-(aq) → Mn2+ (aq) + CO2(9) a. Balance the reaction in acidic solution b. Determine the standard cell potential of the representative voltaic cell c. Determine the standard free energy change of this reaction d. Determine the cell potential if the pH = 4 and all other solute concentrations were standard.
10. Based on E values, what is the strongest reducing and oxidizing agent in each of the following groups. Briefly explain your reasoning. 2+ b. Strongest Oxidizing Agent: dziel, d(aa), MnO4-(1M H*), Mn2+(1M H*), ??(1M H*)
Permanganate, MnO4–, can act as an oxidizing agent in both acidic and basic aqueous solutions. Balance each of the following reactions by the half–reaction method, showing all steps in the balancing process. i. MnO4– + Al ––> MnO2 + Al(OH)4– in aqueous base ii. MnO4– + CH3COOH ––> Mn+2 + CO2 in aqueous acid
An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and will be used in an experiment to determine the percentage of iron in a sample of ammonium iron (II) sulfate hexahydrate. The titration is self-indicating because at the equivalence point the products are a different colour than the original reactants. The two half reactions are: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) Fe^2+(aq) ---> Fe^3+(aq) + e- a) What is a redox...
Which of the following is the strongest oxidizing agent? MnO4 ̄ (aq) + 4 H+ (aq) + 3 e ̄ → MnO2 (s) + 2 H2O (l) I2(aq) +2e ̄ →2I ̄(aq) Zn2+(aq) +2e ̄ →Zn(s) εo = 1.68 V εo =0.54V εo =-0.76V Al Ni Both Al and Ni would work Neither Al nor Ni would work
What is the appropriate weight for the preparation of the required concentrations from the following oxidizing factors? Materials No. of electrons gained Molecular Weight (g/mol) Equivalent Weight (g/eq) Concentration Weight (gm) MnO4 → Mn2+ no. of e = 2N in 300 ml Potassium permanganate KMnO4 Potassium dichromate K2Cr2O7 Cr2O72-→ 2Cr3+ no. of e = 2M in 500 ml lodine 1221 no. of e = 3N in 2000ml molecular weight (g/mol) Equivalent weight of an oxidizing agent = no. of electrons...
Permanganate ion oxidizes hydrogen peroxide in acidic solution according to the following equation: 2 MnO4–(aq) + 5 H2O2(aq) + 6 H+(aq) 2 Mn2+(aq) + 5 O2(g) + 8 H2O(l) If 35.0 mL of an acidic 0.150 M KMnO4 solution is required to consume all the H2O2 in 50.0 mL of a disinfectant solution, what is the concentration of H2O2 in the disinfectant? 0.0420 M 0.105 M 0.263 M 0.368 M When a solution of barium hydroxide is mixed with a...
Question 31 4 pts 31. Determine which is reduced agent? MnO4 (aq) +5Fe2(aq) + 8 H(aq) 5 Fe(aq) + Mn2 (aq) + 4H2O(1) Mn in MnO4- H: Fe3+ Fe2+ Question 30 30. Calculate pH of 0.100 M HNO2(aq). K-2.8 x 10-5 9.01 6.21 2.78 5.21
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. MnO4- + 8H + 5e- → Mn2+ (aq) + 4H2O (+1.51 V) MnO2 + 4H +2e- → Mn2+ (aq) + 2H2O (+1.22 V) xLi+ + C6 + e- → LixC5 (-3.00 V) 1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The reaction...