Question

Calculate the standard cell potential (E∘) for the reaction

X(s)+Y+(aq)→X+(aq)+Y(s)

if K = 6.43×10^−3.

Express your answer numerically in volts.

Answer #1

Calculate the standard cell potential (E∘) for the reaction
X(s)+Y+(aq)→X+(aq)+Y(s) if K = 2.71×10−3.

1) Calculate the standard cell potential (E∘) for the
reaction
X(s)+Y+(aq)→X+(aq)+Y(s)
if K = 1.12×10−3.
2)Calculate the standard cell potential at 25 ∘C for the
reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s)
where ΔH∘ = -573 kJ and ΔS∘ = -415 J/K .

A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at
25 ∘C under each of the following conditions.
1. [Fe3+]= 2.3×10−3 M ; [Mg2+]= 2.90 M
Express your answer in units of volts.
2. [Fe3+]= 2.90 M ; [Mg2+]= 2.3×10−3 M
Express your answer in units of volts.

A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq)
Calculate the cell potential at 25 ∘C under each of the following
conditions.
Part B
[Fe3+]= 1.2×10−3 M ; [Mg2+]= 3.25 M
Express your answer in units of volts.
Part C
[Fe3+]= 3.25 M ; [Mg2+]= 1.2×10−3 M
Express your answer in units of volts.

Calculate the standard potential, E°, for this reaction from its
equilibrium constant at 298 K.
X(s) + Y^2+(aq)----->X^2+(aq) + Y(s) K=6.11x10^-5
<--------

What is the cell potential for the reaction
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 47 ∘C when [Fe2+]= 3.10 M and
[Mg2+]= 0.110 MM . Express the potential numerically in volts.

Calculate the standard cell potential at 25 ∘C for the
reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s)
where ΔH∘ = -793 kJ and ΔS∘ = -143 J/K .

Calculate the standard cell potential at 25 ∘C for the reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -597 kJ and ΔS∘ = -337
J/K

Calculate the standard cell potential for each of the
electrochemical cells. Part A 2Ag+(aq)+Pb(s)?2Ag(s)+Pb2+(aq)
Express your answer using two significant figures. Part B
2ClO2(g)+2I?(aq)?2ClO?2(aq)+I2(s) Express your answer using two
significant figures. Part C
O2(g)+4H+(aq)+2Zn(s)?2H2O(l)+2Zn2+(aq)

Consider the cell: Hg(l) ׀ Hg2SO4(s) ׀ FeSO4(aq) ׀ Fe(s) The
standard cell potential (E θ ) for the reduction of Fe2+ is -0.447
V and the standard cell potential for the reduction of Hg2SO4(s) is
+0.6125 V.
(a) Write the cell reaction.
(b) If the activity of FeSO4(aq) is 0.0100, calculate the cell
potential and the standard Gibbs energy at 25°C.

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