5. Balance the following redox equation using the half-reaction method: MnO41 H2O2 Mn2+ +O2 (acidic medium) Reduction half Mno Mn Oxidation hatf H20, O2 2f 8H MnO H20, 02° 2 t 4H2O No + 2Ht 2/8H 5e 5 (He O 2.1 T + MnOy Mn 4 H2O) + O2 4 2H 2e ) IoHt 10e + 2 Mna 50, t 2Mn2 8 H,O 5 H2O + + 8 HOt50, + 1OH 2Mn2 +8 H20 t50, + IOH lo Ht 2 MnOy- 6. Using the balanced redox equation from question #5, answer the following: A] How many mL of a standard 0.150 M KMnO4 solution are required to react with 0.500 grams of hydrogen peroxide, H2O2? B] A student used 32.47 mL of a 0.150 M potassium permanganate, KMnO4, to react with hydrogen peroxide. How many grams of H2O2 reacted with the KMNO4 solution? 16 Ht t 2 MnO4- + 8 H20 +502 + 10 H 2+ t 2 Mn 197 1l
5. Balance the following redox equation using the half-reaction method: MnO41 H2O2 Mn2+ +O2 (acidic medium) Reduction half Mno Mn Oxidation hatf H20, O2 2f 8H MnO H20, 02° 2 t 4H2O No + 2Ht 2/8H 5e 5 (He O 2.1 T + MnOy Mn 4 H2O) + O2 4 2H 2e ) IoHt 10e + 2 Mna 50, t 2Mn2 8 H,O 5 H2O + + 8 HOt50, + 1OH 2Mn2 +8 H20 t50, + IOH lo Ht 2 MnOy- 6. Using the balanced redox equation from question #5, answer the following: A] How many mL of a standard 0.150 M KMnO4 solution are required to react with 0.500 grams of hydrogen peroxide, H2O2? B] A student used 32.47 mL of a 0.150 M potassium permanganate, KMnO4, to react with hydrogen peroxide. How many grams of H2O2 reacted with the KMNO4 solution? 16 Ht t 2 MnO4- + 8 H20 +502 + 10 H 2+ t 2 Mn 197 1l
Chemistry: An Atoms First Approach
2nd Edition
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Author:Steven S. Zumdahl, Susan A. Zumdahl
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Chapter17: Electrochemistry
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Problem 159MP: A galvanic cell is based on the following half-reactions: In this cell, the copper compartment...
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Question 6 B
![5. Balance the following redox equation using the half-reaction method:
MnO41 H2O2 Mn2+ +O2
(acidic medium)
Reduction half Mno Mn
Oxidation hatf H20, O2
2f
8H MnO
H20, 02°
2 t
4H2O
No
+
2Ht
2/8H 5e
5 (He O
2.1
T
+ MnOy
Mn 4 H2O)
+
O2
4 2H 2e )
IoHt 10e
+ 2 Mna
50, t
2Mn2 8 H,O
5 H2O
+
+ 8 HOt50, + 1OH
2Mn2 +8 H20 t50, + IOH
lo Ht 2 MnOy-
6. Using the balanced redox equation from question #5, answer the following:
A] How many mL of a standard 0.150 M KMnO4 solution are required to react with
0.500 grams of hydrogen peroxide, H2O2?
B] A student used 32.47 mL of a 0.150 M potassium permanganate, KMnO4, to react
with hydrogen peroxide. How many grams of H2O2 reacted with the KMNO4 solution?
16 Ht t 2 MnO4-
+ 8 H20 +502 + 10 H
2+
t
2 Mn
197
1l](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8a30a005-d7e5-458b-b4bc-cfc1eedff542%2F9efc611b-637e-4174-92fa-48873f479f8b%2Ftdy3to.jpeg&w=3840&q=75)
Transcribed Image Text:5. Balance the following redox equation using the half-reaction method:
MnO41 H2O2 Mn2+ +O2
(acidic medium)
Reduction half Mno Mn
Oxidation hatf H20, O2
2f
8H MnO
H20, 02°
2 t
4H2O
No
+
2Ht
2/8H 5e
5 (He O
2.1
T
+ MnOy
Mn 4 H2O)
+
O2
4 2H 2e )
IoHt 10e
+ 2 Mna
50, t
2Mn2 8 H,O
5 H2O
+
+ 8 HOt50, + 1OH
2Mn2 +8 H20 t50, + IOH
lo Ht 2 MnOy-
6. Using the balanced redox equation from question #5, answer the following:
A] How many mL of a standard 0.150 M KMnO4 solution are required to react with
0.500 grams of hydrogen peroxide, H2O2?
B] A student used 32.47 mL of a 0.150 M potassium permanganate, KMnO4, to react
with hydrogen peroxide. How many grams of H2O2 reacted with the KMNO4 solution?
16 Ht t 2 MnO4-
+ 8 H20 +502 + 10 H
2+
t
2 Mn
197
1l
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