Question

What is the calculated value of the cell potential at 298 K for
an electrochemical cell with the following reaction, when the
**H _{2}** pressure is

Answer: _____ V ?

The cell reaction as written above is product-favored (spontaneous) for the concentrations given: _______(true/false)?

Answer #1

i)

0.780V

Explanation

2H^{+}(aq) + Zn(s) ------> H2(g) +
Zn^{2+}(aq)

Reactant quotient, Q = P_{H2} ×
[Zn^{2+}]/[H^{+}]^{2}

Q = 0.005bar × 0^{+}.000342M/(1.46)^{2}

Q = 8.022×10^{-7}

Oxidation half reaction (at anode)

Zn(s) ------->
Zn^{2+}(aq) + 2e E°_{red} = - 0.762V

Reduction half reaction (at cathode)

2H^{+}(aq) + 2e
--------> H2(g) E°_{red} = 0.000V

E°_{cell} =
E°_{red,cathode} - E°_{red,anode} = 0.000V - (-
0.762V) = 0.762V

Number of electron transfer ,n = 2

at 25°C , Nernst equation is as follows

E_{cell} =
E°_{cell} - (0.0592V/n)logQ

E_{cell} = 0.762V -
(0.0592V/2)log(8.022×10^{-7})

E_{cell} = 0.762V +
0.18V

E_{cell} =
0.780V

ii)

True

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...

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 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 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?

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

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 standard cell potential for an electrochemical cell
based on the following half-reactions?
IO3-(aq) + 6 H+(aq) + 6 e- ----> I-(aq) + 3 H2O(l ) E° =
1.085 V
Zn2+(aq) + 2 e- ---> Zn(s) E° = -0.762 V

Consider an electrochemical cell based on the following
reaction:
Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq) + H2(g)
All dissolved species are at 2.5 x 10-3 M; pressure of H2 is 1
bar (standard state) Use the Nernst equation to calculate E.

Write the cell notation for an electrochemical cell consisting
of an anode where Ni(s) is oxidized to Ni2+(aq) and a cathode where
Fe3+(aq) is reduced to Fe2+(aq) at a platinum electrode. Assume all
aqueous solutions have a concentration of 1 mol/L and gases have a
pressure of 1 bar.
Write the cell notation for an electrochemical cell consisting
of an anode where Zn (s) is
oxidized to Zn2+(aq)
and a cathode where
Ag+(aq) is reduced to
Ag (s) . Assume...

Electrochemical Cell Potentials
Table 1: Electrochemical
Cell Potentials
Cell
Measured Total Potential
from Multimeter (V)1
Individual Half-Cell
Potentials
Cell
Reactions5
ΔG
(kJ)6
(Cu) Electrode Standard
Potential (V)2
Metal Electrode
Experimental
Potential
(V)3
Metal Electrode
Theoretical
Potential
(V)4
Metal Electrode
Potential
% Error
Cu | Sn
0.469
0.34 V
0.34-0.469
=-0.129
Cathode:
Cu2+ + 2e- -> Cu
Anode:
Sn ->Sn2++ 2e-
Net:
Cu2+ + Sn -> Cu + Sn2+
Cu | Al
0.796
0.34 V
0.34-0.796
=-0.456
Cathode:
Cu2+ +...

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