Question

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

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 the following reaction, when the
**H _{2}** pressure is

Answer: _____ V

The cell reaction as written above is spontaneous for the
concentrations given: _____ ( TRUE/FALSE )

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

Answer: _____ V

The cell reaction as written above is spontaneous for the
concentrations given: _____ ( TRUE/FALSE )

Answer #1

**Cl _{2}**

Pb-------------------> Pb^{+2} +
2e^{-}
E0 = 0.13V

Cl2 +2e^{-} --------> 2Cl^{-}
E0 = 1.36v

----------------------------------------------------------------------------

Pb(s)+ Cl2(g) ----------> Pb^{+2} (aq) +
2Cl^{-} (aq) Eocell = 1.49v

G^{0} =
-nE0cell*F

= -2*1.49*96500 = -287570J

G^{0}
<0 spontaneous reaction

Ecell = Ecell -0.0592/n
log[Cl^{-}]^{2} [Pb^{+2}]/PCl2

=
1.49-0.0592/2 log(1.48)^{2}*(1.07)/8.15*10^{-4}

= 1.49-0.0296*3.4587

= 1.39v

**2****H ^{+}**

Ni(s) ---------------> Ni^{+2} +
2e^{-} E0 =
0.23v

2H^{+} + 2e^{-} -------->
H2
E0 = 0.0v

-------------------------------------------------------------

**2****H ^{+}**

G^{0} =
-nE0cell*F

= -2*0.23*96500 = -44390J

G^{0}
<0 spontaneous reaction

Ecell = E0cell -0.0592/n logQ

=
0.23-0.0592/2 log[Ni^{+2}]PH2/[H+]^{2}

=
0.23-0.0296log3.76*10^{-4}
*5.72*10^{-3}/(1.29)^{2}

= 0.23-0.0296*-5.8886 = 0.404v

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 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 1.44 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 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 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)?

When [ Pb2+] = 1.00
M, the observed cell potential at 298K for an electrochemical cell
with the reaction shown below is 1.611 V. What is
the Al3+concentration in this
cell?
3
Pb2+(aq) +
2 Al (s)
----> 3 Pb
(s) + 2
Al3+(aq)
[ Al3+] = ______M

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 OCP (open circuit potential) of the H2(g)/Cl2(g)
electrochemical cell [Pt(s)|H2(g)|HCl(aq)|Cl2(g)|Pt(s)] at 25 oC,
if partial pressure of hydrogen and chlorine are 0.5 bar and the
concentration of HCl(aq) is 5 mol/kg?

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