The amount of hydrogen peroxide in a sample may be determined by reacting it quantitatively with permanganate ions as illustrated in the redox reaction below: MnO4+H₂O₂ → O₂ + Mn²+ The analysis is usually done in acidic conditions to prevent the precipitation of manganese dioxide Which of the following is the correct balanced redox reaction in acidic medium? Ⓒa. 2MnO² +5H₂O₂ → 50₂ + 2Mn²+ + 2H₂O +60H¯ b. MnO4 + 2H₂O₂ → 30₂ + Mn²+ + 2H₂O c. 2MnO² +5H₂O₂ + 6H+ → 50₂ + 2Mn²+ +8H₂O O d. 2Mn0 +5H₂O₂ + 3H₂ → 50₂ +2Mn²+ +8H₂0

The amount of hydrogen peroxide in a sample may be determined by reacting it quantitatively with permanganate ions as illustrated in the redox reaction below: MnO4+H₂O₂ → O₂ + Mn²+ The analysis is usually done in acidic conditions to prevent the precipitation of manganese dioxide Which of the following is the correct balanced redox reaction in acidic medium? Ⓒa. 2MnO² +5H₂O₂ → 50₂ + 2Mn²+ + 2H₂O +60H¯ b. MnO4 + 2H₂O₂ → 30₂ + Mn²+ + 2H₂O c. 2MnO² +5H₂O₂ + 6H+ → 50₂ + 2Mn²+ +8H₂O O d. 2Mn0 +5H₂O₂ + 3H₂ → 50₂ +2Mn²+ +8H₂0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Write a balanced net ionic equation for a redox reaction that results in the formation of potassium chloride. (Assume that potassium chloride is not a starting material, and assume the reaction takes place in aqueous solution.) X, Не (aq), 2K(ag)+Cl, (aq) KCI(aq)
Complete and balance the following redox reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. ReO₄⁻(aq) + MnO₂(s) → Re(s) + MnO₄⁻(aq)
In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: 3Ag + Cr³+→→→→Cr + 3Ag+ formula of the oxidizing agent: name of the element reduced: formula of the reducing agent:
The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction is given below. 2 H2O(l) + 2 e− → H2(g) + 2 OH− (aq) Hydroxide ion reacts with lactic acid as soon as it is produced. The endpoint of the reaction is detected with an acid-base indicator. It required 104 s for a current of 13.1 mA to reach the endpoint. How many grams of lactic acid (a monoprotic acid) were present in the sample?
Identify whether each of the following reaction is a redox reaction. If it is so, by showing the change in oxidation numbers identify the oxidizing agent and reducing agent. 4 CaSO3 ⟶ 3 CaSO4 + CaS 2 KMnO4+ 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2
In the balanced redox reaction: 2 Cu(s) + S(s) > Cu 2S(s); how many electrons are gained or lost by each copper atom?
Balance the following redox reaction that occurs in a basic solution: N₂O₄(aq) + TeO₃²⁻(aq) → Te(s) + NO₃¹⁻(aq))
A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):
c. For the unbalanced redox reaction Cu + 10 ➜→ Cu²+ + 1₂ Which is oxidizing agent (oxidant)? Write the balanced redox net ionic equation when the reaction is conducted in an acidic solution.
Balance the following reaction using the half-reaction method, in both acidic and basic conditions. Cr(OH)3 + Br2 → CrO42−+Br− When balanced, determine the entity which is reduced, the entity which is oxidized, the reducing agent and the oxidizing agent.
The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.