Question

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn 2 ] = 0.768 M and [Sn2 ] = 0.0200 M. Standard reduction potentials can be found here. Zn(s)+Sn2+(aq)----->Zn2+(aq)+Sn(s)

Zn+2e- ---->Zn = -0.76

Sn+ + 2e- ----> Sn = -0.14

Answer #1

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Zn2 ] = 0.821 M and [Ni2 ] =
0.0200 M. Standard reduction potentials can be found here.
Zn(s) + Ni+2(aq)=Zn+2(aq) + Ni(s)

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Mg2 ] = 0.830 M and [Sn2 ] =
0.0140 M. Standard reduction potentials can be found here.
Mg(s) + Sn2+ (aq) <--> Mg2+ (aq) + Sn(s)
Standard... Mg2+(aq) + 2e– → Mg(s.....–2.38
Sn4+(aq) +2e– → Sn2+(aq)....+0.151

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Cr2 ] = 0.864 M and [Sn2 ] =
0.0190 M. Standard reduction potentials can be found here.
Cr(s)+Sn^2+(aq) forward and reverse arrow Cr^2+(aq)+Sn(s)

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Zn2 ] = 0.837 M and [Fe2 ] =
0.0100 M. Standard reduction potentials can be found here.
Zn(s)+Fe^2+(aq) <--->Zn^2+(aq)+Fe(s)
E= _______ V

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Cr2 ] = 0.870 M and [Sn2 ] =
0.0190 M. Standard reduction potentials can be found here.
Cr + Sn2+ <==> Cr2+ + Sn
E= ??V

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Cr2 ] = 0.893 M and [Ni2 ] =
0.0130 M. Standard reduction potentials can be found here.
Cr (s) + Ni^2+ (aq) --> <-- Cr^2+ (aq) + Ni (s)

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Mg2 ] = 0.887 M and [Sn2 ] =
0.0150 M. Mg(s)+Sn2+(aq)------->Mg2+ (aq)+Sn(s)

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Zn2 ] = 0.771 M and [Ni2 ] =
0.0200 M.

Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Zn2 ] = 0.752 M and [Sn2 ] =
0.0170 M

The following cell has a potential of 0.040 V at 25°C.
Zn(s)∣Zn2+(aq) || Cr3+(0.020 M) | Cr(s) What is the concentration
of Zn2+? The standard reduction potentials are given below:
Zn2+(aq) + 2e− → Zn(aq) Eo = − 0.760 Cr3+(aq) + 3e− → Cr(s) V Eo =
− 0.740 V

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