Question

Calculate the open circuit potential of a Daniell cell (at 25 oC and 1 bar) with ZnSO4(aq, 0.01 mol/kg ) on the left hand side and CuSO4(aq, 0.002 mol/kg) on the right hand side if the ionic activity coefficients of Cu2+(aq) and Zn2+(aq) are, respectively, 0.658 and 0.392.

Answer #1

Cu is cathode & Zn is anode

Cu^{2+}(aq)+2e^{-}-->Cu(s)

Zn(s)-->Zn^{2+}(aq)+2e^{-}

note that n=2 for this cell

activities for solid materials is one

=

& =1

therefore

on substing all values

E= 1.1-8.314*298/(2*96 485.3329)ln(0.392*0.01/(0.658*0.002)=1.088V

so open circuit potential is **1.088V**

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?

Consider the Daniell cell, for which the overall cell reaction
is Zn(s)+Cu2+(aq)⇌Zn2+(aq)+Cu(s) The concentrations of CuSO4 and
ZnSO4 are 2.20×10−3 m and 1.10×10−3 m , respectively.
Part A
Calculate E setting the activities of the ionic species equal to
their molalities.
Express your answer to four significant figures and include the
appropriate units.
E = ?
Part B
Calculate γ±,ZnSO4 for the half-cell solutions using the
Debye-Huckel limiting law.
Express your answer using three significant figures.
γ±,ZnSO4 = ?
Part...

State true or false for the folloing statements.
1. The Faraday constant equals the charge of one proton.
2. In the spontaneous chemical reaction of an electrochemical
cell, electrons flow from the anode to the cathode.
3. Increasing the activity of a reactant in the cell's chemical
reaction must increase the cell potential.
4. If we double all the coefficients in a cell's reaction, the
number of electrons transferred, n, is doubled but the
cell potential is unchanged.
5. The...

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