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76. An electrochemical cell is based on these two half-reactions: Ox: Sn(s) — Sn2+ (aq, 2.00 M) + 2e Red: ClO2(g, 0.100 atm) + CIO2 (aq, 2.00 M) Calculate the cell potential at 25°C.

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Related questions

For the following electrochemical cell Sn(s)|Sn2+ (aq, 0.0155 m)||Ag+ (aq, 1.50 m)|Ag(s), what is the net cell equation?

Calculate the following values at 25°C using standard potentials as needed.

  •  
  •  
  •  
  •  

1 ) 2.52×10−2 L sample of a solution of Cu +requires 3.28×10−2 L of 0.133 M KMnO4solution to reach the equivalence point. The products of the reaction are Cu2+ and Mn2+.

2) An electrochemical cell is based on the following two half-reactions:
Ox: Sn(s)→Sn2+(aq, 1.50 M )+2e−
Red:ClO2(g, 0.105 atm )+e−→ClO−2(aq, 1.50 M)

Compute the cell potential at 25 ∘C.

3 ) A 115.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with a 225.0 −mL sample of a solution that is 0.14 M in NaCN.

After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

4)55.0 mL of 0.17 M HCHO2 with 75.0 mL of 0.11 M NaCHO2

5 ) 130.0 mL of 0.10 M NH3 with 250.0 mL of 0.10 M NH4Cl

CALCULATE THE PH FOR 4 ND 5

Part A

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.

Sn(s) | Sn2+(aq, 0.022 M) || Ag+(aq, 2.7 M) | Ag(s)


Sn2+(aq)+2e−→Sn(s) Eo=−0.14V
Ag+(aq)+1e1→Ag(s) Eo=0.80V

1.01 V
-0.83 V
-0.66 V
0.01 V
1.31 V

Part B

How many electrons are transferred in the following reaction? (The reaction is unbalanced.)

Mg(s) + Al3+(aq) → Al(s) + Mg2+(aq)

3
6
1
2
4

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