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Redox
Related Topics
Wize University Chemistry Textbook > Electrochemistry
Redox Reactions
4 Activities
C
2
O
4
2−
(aq) + MnO
4
−
(aq) → CO
3
2−
(aq) + MnO
2
(s)
Which one is the reducing agent in this equation?
C
2
O
4
2−
MnO
4
−
Not a redox reaction
CO
3
2−
MnO
2
I don't know
Check Submission
More Redox Reactions Questions:
Electrochemistry: Redox
What is the reducing agent in the following unbalanced chemical reaction?
NO + Au
+
→ NO
3
-
+ Au
Consider the following balanced redox equation:
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
Which species is the reducing agent?
Consider the following balanced redox equation:
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
Which species is the oxidizing agent?
Consider the following balanced redox equation:
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
Which species is being reduced?
Consider the following balanced redox equation:
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
Which species is being oxidized?
Consider the following balanced redox equation:
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
16H^+_{(aq)}+2MnO^-_{4(aq)}+10Cl^-_{(aq)} \to 2Mn^{2+}_{(aq)}+5Cl_{2(g)}+8H_2O_{(l)}
16
H
(
a
q
)
+
+
2
M
n
O
4
(
a
q
)
−
+
10
C
l
(
a
q
)
−
→
2
M
n
(
a
q
)
2
+
+
5
C
l
2
(
g
)
+
8
H
2
O
(
l
)
Would you use an oxidizing or reducing agent for the following reaction to occur?
SO
4
2-
--> S
2-
What product forms at each electrode in the aqueous electrolysis of the following salts? Ignore overpotential effects.
LiF
SnSO
4
A concentration cell consists of two H
2
/H
+
half-cells. Half-cell A has H
2
at 0.90 atm bubbling into 0.10 M HCl. Half-cell B has H
2
atm bubbling into 2.0 M HCl. Which half-cell houses the anode? What is the voltage of this cell?
Similar to Practice Exam 1 Fall 2018 (CHM 2045 UF)
What is the oxidizing agent in the following unbalanced chemical reaction?
NO + Au
+
→ NO
3
-
+ Au