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Lesson Worksheet: Electrochemical Cell Potential Chemistry • 10th Grade

In this worksheet, we will practice calculating the standard cell potential of galvanic cells using values from the electrochemical series.

Q1:

Find, to 3 decimal places, the standard cell potential for the galvanic cell with the following overall reaction: 2Ag()+Fe()2Ag()+Fe()+2+aqssaq

Half-EquationAg()+eAg()+aqsFe()+2eFe()2+aqs
Standard Electrode Potential, 𝐸 (V)+0.79960.447

Q2:

A galvanic cell consists of a Mg electrode in 1 MMg(NO)32 solution and a Ag electrode in 1 MAgNO3 solution. What is the standard cell potential?

Half-Equation Mg()+2eMg()2+aqsAg()+eAg()+aqs
Standard Electrode Potential, 𝐸 (V)2.372+0.7996

Q3:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell consisting of Au3+/Au and Ni2+/Ni half-cells.

Half-EquationAu()+3eAu()3+aqsNi()+2eNi()+aqs
Standard Electrode Potential, 𝐸 (V)+1.4980.257
  • A1.241 V
  • B1.755 V
  • C1.755 V
  • D1.241 V

Q4:

Using the standard electrode potentials in the table below, calculate the standard cell potential for a galvanic cell with the following overall reaction: Sn()+2Cu()Sn()+2Cu()saqaqaq2+2++

Half-Equation Sn()+2eSn()2+aqsCu()+eCu()2++aqaq
Standard Electrode Potential, 𝐸 (V)0.1375+0.153

Q5:

Using the standard electrode potentials shown in the table, calculate, to 3 decimal places, the cell potential for the following electrochemical cell: Cd()|Cd(,1M)Ni(,1M)|Ni()saqaqs2+2+

Half-EquationCd()+2eCd()2+aqsNi()+2eNi()2+aqs
Standard Electrode Potential, 𝐸()V0.40300.257
  • A+0.146V
  • B+0.660 V
  • C0.660 V
  • D0.146 V
  • E+0.164 V

Q6:

Using the standard electrode potentials shown in the table, determine which of the following metals are capable of reducing LaO23 to La metal.

Half-EquationCa()+2eCa()2+aqsAl()+3eAl()3+aqsFe()+2eFe()2+aqsLa()+3eLa()3+aqs
Standard Electrode Potential, 𝐸 (V)2.8681.6620.4472.52
  • AAl only
  • BCa only
  • CFe only
  • DAl and Fe
  • ECa and Al

Q7:

The figure shows the setup of a voltaic cell.

What one of the following is the correct expression of the setup in cell notation?

  • ACu(,1M)Cu()Ag(,1M)Ag()2++aqsaqs
  • BCu(,1M)Cu()Ag()Ag(,1M)2++aqssaq
  • CCu()Cu(,1M)Ag()Ag(,1M)saqsaq2++
  • DCu()Cu(,M)Ag(,M)Ag()saqaqs112++
  • EAg(,1M)Ag()Cu()Cu(,1M)+2+aqssaq

Q8:

Concentrated hydrochloric acid is not used to acidify the dichromate ions in the oxidation of a primary alcohol to a carboxylic acid. In practice, the dichromate oxidizes the chloride ions, so sulfuric acid is used instead.

The half-equations and standard electrode potentials for this oxidation are shown:

Cl+2e2ClVCrO+14H+6e2Cr+7HOV2272+3+2𝐸=+1.36𝐸=+1.33

What would the standard cell potential for a galvanic cell consisting of these two half-cells be?

Is the reaction feasible according to previous calculation? How does this explain the choice of acid in the experiment discussed?

  • AThe reaction is feasible and concentrated hydrochloric acid would have a more negative electrode potential (<+1.36V), making the oxidation of chloride ions by dichromate ions also feasible.
  • BThe reaction is not feasible; however, concentrated hydrochloric acid would have a more negative electrode potential (<+1.36V), making the oxidation of chloride ions by dichromate ions feasible.
  • CThe reaction is feasible and concentrated hydrochloric acid would have a more positive electrode potential (>+1.36V), making the oxidation of chloride ions by dichromate ions also feasible.
  • DThe reaction is not feasible; however, concentrated hydrochloric acid would have a more positive electrode potential (>+1.36V), making the oxidation of chloride ions by dichromate ions feasible.

Q9:

The following is a simplified diagram of a cell, which combines a half-cell of silver wire in a 1 M solution of silver ions paired with a half-cell of an unknown metal, M, in a 1 M solution of its ions.

The silver electrode is found to be the positive electrode. Which of the arrows on the diagram shows the correct direction in which electrons would flow in this circuit?

  • AA
  • BB

Given that the standard cell potential was found to be +1.0496 V and that the standard electrode potential of the silver half-cell is known to be +0.7996 V, what is the standard electrode potential of the M()M(,1M)saq|2+ half-cell?

Q10:

The standard electrode potential of a copper half-cell, where a copper metal electrode is placed in a solution of copper 2+ ions, is known to be +0.337 V.

What is the standard cell potential when this copper half-cell is connected to a similar half-cell of Zn metal and Zn2+ ions that has a standard electrode potential of 0.7618 V?

This lesson includes 31 additional questions and 21 additional question variations for subscribers.

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