Question

When [ **Pb ^{2+}**] =

[

Answer #1

When the Cu2+ concentration is
1.40 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
2.805V. What is the
Mg2+ concentration?
Cu2+(aq) +
Mg(s) ----->
Cu(s) +
Mg2+(aq)
Answer: ______M

A) When the Cu2+ concentration is
1.07 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
1.607V. What is the
Mn2+ concentration?
Cu2+(aq) +
Mn(s)-->
Cu(s) +
Mn2+(aq)
Answer: _____ M
B) When the Cu2+ concentration is
5.71×10-4 M, the observed cell
potential at 298K for an electrochemical cell with the following
reaction is 2.609V. What is the
Mg2+ concentration?
Cu2+(aq) +
Mg(s)--->
Cu(s) +
Mg2+(aq)
Answer: _____ M
C) When the Cu2+...

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Pb2+
concentration is 1.20 M and the Mn2+ concentration is 5.43×10-4 M
?
Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq)
Answer: in V
The cell reaction as written above is spontaneous for the
concentrations given: true or false?

A) What is the calculated value of the cell potential at 298K
for an electrochemical cell with the following reaction, when the
Cl2 pressure is
8.15×10-4 atm, the
Cl- concentration is
1.48M, and the Pb2+
concentration is 1.07M ?
Cl2(g) +
Pb(s) --->
2Cl-(aq)
+ Pb2+(aq)
Answer: _____ V
The cell reaction as written above is spontaneous for the
concentrations given:____ ( TRUE/FALSE )
B)What is the calculated value of the cell potential at 298K for
an electrochemical cell with...

1. What is the calculated value of the cell potential at 298K
for an electrochemical cell with the following reaction, when the
Pb2+ concentration is
4.09×10-4 M and the
Mg2+ concentration is
1.03 M ?
Pb2+(aq) +
Mg(s) --->
Pb(s) +
Mg2+(aq)
Answer: ___V
The cell reaction as written above is spontaneous for the
concentrations given____. (true or false)
(From the table of standard reduction potentials: )
Pb2+(aq) + 2 e- --> Pb(s)
-0.126
Mg2+(aq) + 2 e- --> Mg(s)...

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 7.38×10-4 M and the Al3+ concentration is 1.43 M
?
3Cu2+(aq) + 2Al(s)3Cu(s) + 2Al3+(aq)
Answer: V
The cell reaction as written above is spontaneous for the
concentrations given: True or False?

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 1.23 M and the Cr3+ concentration is 5.82×10-4 M ?
3Cu2+(aq) + 2Cr(s)-->3Cu(s) + 2Cr3+(aq) Answer: V The cell
reaction as written above is spontaneous for the concentrations
given

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 1.44 M and the Mg2+ concentration is 1.47×10-4 M
?
Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)
Answer: V
The cell reaction as written above is spontaneous for the
concentrations given:
_______
true
false

Consider an electrochemical cell, where [Cr2+] = 0.15
M and [Al3+] = 0.0040 M, based on the following
reaction:
3
Cr2+(aq) + 2 Al(s) → 3
Cr(s) + 2 Al3+(aq)
The standard reduction potentials are as follows:
Cr2+(aq) + 2
e- → Cr(s) E° = -0.91 V
Al3+(aq) + 3
e- → Al(s) E° = -1.66 V
What is the cell potential at 25 °C?
Select one:
a. 0.71 V
b. 0.73 V
c. 0.75 V
d. 0.77 V
Can you please hsow working :)

What is the calculated value of the cell potential at 298 K for
an electrochemical cell with the following reaction, when the
H2 pressure is
5.00×10-3 bar, the
H+ concentration is
1.46 M, and the
Zn2+concentration is
3.42×10-4 M ?
2H+(aq)
+ Zn(s) ---->
H2(g) +
Zn2+(aq)
Answer: _____ V ?
The cell reaction as written above is product-favored (spontaneous)
for the concentrations given: _______(true/false)?

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