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The cell Fe(s) mid Fe²⁺(aq) ∥ Cu²⁺(aq) mid Cu(s) has E°… | StemPy Lab
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The cell Fe(s) mid Fe²⁺(aq) ∥ Cu²⁺(aq) mid Cu(s) has E° = 0.78 V and n = 2 at 298 K. At one moment its emf is 0.85 V. What is the reaction quotient Q at that moment?
Chemistry
Medium
High School (11–12)
Electrochemistry › Galvanic Cells, Electrode Potential and the Nernst Equation
Board Exam
AP
A-Level
IB
Created by
StemPy Lab
The cell
Fe
(
s
)
∣
Fe
2
+
(
a
q
)
∥
Cu
2
+
(
a
q
)
∣
Cu
(
s
)
\text{Fe}(s) \mid \text{Fe}^{2+}(aq) \parallel \text{Cu}^{2+}(aq) \mid \text{Cu}(s)
Fe
(
s
)
∣
Fe
2
+
(
a
q
)
∥
Cu
2
+
(
a
q
)
∣
Cu
(
s
)
has
E
∘
=
0.78
V
E^\circ = 0.78\ \text{V}
E
∘
=
0.78
V
and
n
=
2
n = 2
n
=
2
at
298
K
298\ \text{K}
298
K
. At one moment its emf is
0.85
V
0.85\ \text{V}
0.85
V
. What is the reaction quotient
Q
Q
Q
at that moment?
4.3
×
10
−
3
4.3 \times 10^{-3}
4.3
×
1
0
−
3
0.065
0.065
0.065
0.85
0.85
0.85
2.3
×
10
2
2.3 \times 10^{2}
2.3
×
1
0
2
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← For the cell Fe(s) mid Fe²⁺(aq) ∥ Cu²⁺(aq) mid Cu(s) with E° = 0.78 V, which Nernst equation is correct at 298 K?
A silver electrode dips into silver nitrate solution at 0.0070 mol/L at 298 K. Use E°(Ag⁺/Ag) = 0.80 V. What is the electrode potential? →
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Electrochemistry › Galvanic Cells, Electrode Potential and the Nernst Equation
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