Question 1

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H2(g)$\rightarrow$ 2Au(s)+ 2H+(aq)+ 2Cl-(aq)

Accepted Answer

Question 2

Use the following diagram of a cell to answer questions  
-In the cell shown above,A is a standard Zn2+/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,which half-reaction occurs in the left-hand cell compartment?

Accepted Answer

A) Zn2+(aq)+ 2e- $\rightarrow$  Zn(s) 
B) Zn(s)$\rightarrow$  Zn2+(aq)+ 2e-  
A) Zn2+(aq)+ 2e- $\rightarrow$  Zn(s) 
B) Zn(s)$\rightarrow$  Zn2+(aq)+ 2e-

Question 3

Of the following five ions or molecules,which is the strongest reducing agent?

Accepted Answer

A) Fe2+ 
B) Cr2+  
C) F-  
D) H2  
E) Co2+  
A) Fe2+ 
B) Cr2+  
C) F-  
D) H2  
E) Co2+

Question 4

Calculate E for the half-reaction below. 2H+(aq,1.00 * 10-5 M)+ 2- $\rightarrow$ H2(g,1.00 atm)

Accepted Answer

A) 0 V 
B) +0.592 V 
C) -0.592 V 
D) -0.296 V 
E) +0.296 V 
A) 0 V 
B) +0.592 V 
C) -0.592 V 
D) -0.296 V 
E) +0.296 V

Question 5

In a working electrochemical cell (+ cell voltage),the cations in the salt bridge move toward the cathode.

Accepted Answer

A) True 
 B)False

Question 6

Use the following diagram of a cell to answer questions  
-In the cell shown above,A is a standard Zn2+/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,what is the equation for the cell reaction?

Accepted Answer

A) Zn2+(aq)+ H2(g)$\rightarrow$  Zn(s)+ 2H+(aq) 
B) Zn(s)+ 2H+(aq)$\rightarrow$  Zn2+(aq)+ H2(g) 
A) Zn2+(aq)+ H2(g)$\rightarrow$  Zn(s)+ 2H+(aq) 
B) Zn(s)+ 2H+(aq)$\rightarrow$  Zn2+(aq)+ H2(g)

Question 7

When a sample of an unknown metal is dropped into 1 M H+(aq)under standard conditions,bubbles are observed.The unknown metal could be silver.

Accepted Answer

A) True 
 B)False

Question 8

Which pair of metals will dissolve in nitric acid?

Accepted Answer

A) Pt,Ag 
B) Pt,Au 
C) Ag,Fe 
D) Ag,Au 
E) Pt,Fe 
A) Pt,Ag 
B) Pt,Au 
C) Ag,Fe 
D) Ag,Au 
E) Pt,Fe

Question 9

What reaction occurs at the cathode in the following cell diagram?
Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l)

Accepted Answer

Hg<sub>2</sub>SO<sub

Question 10

How many moles of O2(g)are produced by electrolysis of Na2SO4(aq)if 0.120 A is passed through the solution for 65.0 min?

Accepted Answer

A) 0.001 21 mol 
B) 0.000 080 8 mol 
C) 0.002 42 mol 
D) 0.004 85 mol 
E) 0.000 020 2 mol 
A) 0.001 21 mol 
B) 0.000 080 8 mol 
C) 0.002 42 mol 
D) 0.004 85 mol 
E) 0.000 020 2 mol

Question 11

The equilibrium constant for the reaction 2Hg(l)+ 2Cl-(aq)+ Ni2+(aq)$\rightarrow$ Ni(s)+ Hg2Cl2(s)
Is 5.6 * 10-20 at 25S1U1P1$\circ$S1S1P0C.Calculate the value of ES1U1P1$\circ$S1S1P0 for a cell utilizing this reaction.

Accepted Answer

A) +0.57 V 
B) -0.25 V 
C) +1.14 V 
D) -1.14 V 
E) -0.57 V 
A) +0.57 V 
B) -0.25 V 
C) +1.14 V 
D) -1.14 V 
E) -0.57 V

Question 12

Consider the following cell:
Pt|Fe2+(aq,0.50 M),Fe3+(aq,0.30 M)m Fe3+(aq,0.035 M),Fe2+(aq,0.010)|Pt
The standard potential for the Fe3+/Fe2+ couple is +0.77 V.Calculate the cell voltage at 25S1U1P1$\circ$S1S1P0C.

Accepted Answer

The answer of Consider the following cell:
Pt|Fe2+(aq,0.50 M),Fe3+(aq,0.30 M)m Fe3+(aq,0.035...

Question 13

For the cell diagram
Pt|H2(g)|H+(aq)mCo3+(aq),Co2+(aq)|Pt
write the reaction that occurs at the cathode.

Accepted Answer

Co³⁺(aq)+

Question 14

For the cell diagram Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l)
What reaction occurs at the cathode?

Accepted Answer

A) CdSO4(s)+ 2e-$\rightarrow$2Cd(s)+ SO42-(aq) 
B) 2Hg(l)+ SO42-(aq)$\rightarrow$ Hg2SO4(s)+ 2e- 
C) 2Cd(s)+ SO42-(aq)$\rightarrow$CdSO4(s)+ 2e- 
D) Hg2SO4(s)+ 2e- $\rightarrow$ 2Hg(l)+ SO42-(aq) 
E) None of the above. 
A) CdSO4(s)+ 2e-$\rightarrow$2Cd(s)+ SO42-(aq) 
B) 2Hg(l)+ SO42-(aq)$\rightarrow$ Hg2SO4(s)+ 2e- 
C) 2Cd(s)+ SO42-(aq)$\rightarrow$CdSO4(s)+ 2e- 
D) Hg2SO4(s)+ 2e- $\rightarrow$ 2Hg(l)+ SO42-(aq) 
E) None of the above.

Question 15

How many moles of Cl2(g)are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,the "chloralkali" process,is 2NaCl(aq)+ 2H2O(l)$\rightarrow$ 2NaOH(aq)+ H2(g)+ Cl2(g)

Accepted Answer

A) 0.0745 mol 
B) 0.149 mol 
C) 0.447 mol 
D) 0.00248 mol 
E) 0.298 mol 
A) 0.0745 mol 
B) 0.149 mol 
C) 0.447 mol 
D) 0.00248 mol 
E) 0.298 mol

Question 16

Use the following to answer questions  
-The galvanic cell shown above uses the half-cells Mg2+/Mg and Zn2+/Zn,and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.Identify A and write the half-reaction that occurs in that compartment.Does the size of the electrode A increase or decrease during operation of the cell? What is the voltmeter reading?

Accepted Answer

A is Mg(s); Mg(s)@#LAT-DLM& Mg

Question 17

What is the proper cell diagram for the reaction 2AgCl(s)+ H2(g)$\rightarrow$  2Ag(s)+ 2H+(aq)+ 2Cl-(aq)

Accepted Answer

Question 18

Given: Ag+(aq)+ e- $\rightarrow$ Ag(s)
E° = 0.80 V
Fe3+(aq)+ e- $\rightarrow$ Fe2+(aq)
ES1U1P1$\circ$S1S1P0 = 0.77 V
Cu2+(aq)+ 2e- $\rightarrow$ Cu(s)
ES1U1P1$\circ$S1S1P0= 0.34 V
Which is the strongest reducing agent?

Accepted Answer

A) Ag 
B) Cu2+  
C) Cu 
D) Ag+  
E) Fe2+  
A) Ag 
B) Cu2+  
C) Cu 
D) Ag+  
E) Fe2+

Question 19

If the standard potential for Cu2+(aq)/Cu+(aq)is 0.15 V and the standard potential for Cu2+(aq)/Cu(s)is 0.34 V,calculate the standard potential for Cu+(aq)+ e- $\rightarrow$ Cu(s).

Accepted Answer

A) +0.32 V 
B) +0.64 V 
C) +0.53 V 
D) +0.83 V 
E) +0.49 V 
A) +0.32 V 
B) +0.64 V 
C) +0.53 V 
D) +0.83 V 
E) +0.49 V

Question 20

The standard potential of the cell Pb(s)|PbSO4(s)|SO42-(aq)m Pb2+(aq)|Pb(s)
Is +0.23 V at 25S1U1P1$\circ$S1S1P0C.Calculate the equilibrium constant for the reaction of 1 M Pb2+(aq)with 1M SO42-(aq).

Accepted Answer

A) 3.7 * 1016  
B) 8.0 * 1017  
C) 6.0 * 107  
D) 1.7 * 10-8  
E) 7.7 * 103  
A) 3.7 * 1016  
B) 8.0 * 1017  
C) 6.0 * 107  
D) 1.7 * 10-8  
E) 7.7 * 103

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H₂(g) $\rightarrow$ 2Au(s)+ 2H⁺(aq)+ 2Cl^-(aq)

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn²⁺/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,which half-reaction occurs in the left-hand cell compartment?

Of the following five ions or molecules,which is the strongest reducing agent?

Calculate E for the half-reaction below. 2H⁺(aq,1.00 * 10^-⁵ M)+ 2^- $\rightarrow$ H₂(g,1.00 atm)

In a working electrochemical cell (+ cell voltage),the cations in the salt bridge move toward the cathode.

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn²⁺/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,what is the equation for the cell reaction?

When a sample of an unknown metal is dropped into 1 M H⁺(aq)under standard conditions,bubbles are observed.The unknown metal could be silver.

Which pair of metals will dissolve in nitric acid?

What reaction occurs at the cathode in the following cell diagram? Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l)

How many moles of O₂(g)are produced by electrolysis of Na₂SO₄(aq)if 0.120 A is passed through the solution for 65.0 min?

The equilibrium constant for the reaction 2Hg(l)+ 2Cl^-(aq)+ Ni²⁺(aq) $\rightarrow$ Ni(s)+ Hg₂Cl₂(s) Is 5.6 * 10^-20 at 25^$\circ$C.Calculate the value of E^$\circ$ for a cell utilizing this reaction.

Consider the following cell: Pt|Fe²⁺(aq,0.50 M),Fe³⁺(aq,0.30 M)m Fe³⁺(aq,0.035 M),Fe²⁺(aq,0.010)|Pt The standard potential for the Fe³⁺/Fe²⁺ couple is +0.77 V.Calculate the cell voltage at 25^$\circ$C.

For the cell diagram Pt|H₂(g)|H⁺(aq)mCo³⁺(aq),Co²⁺(aq)|Pt write the reaction that occurs at the cathode.

For the cell diagram Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l) What reaction occurs at the cathode?

How many moles of Cl₂(g)are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,the "chloralkali" process,is 2NaCl(aq)+ 2H₂O(l) $\rightarrow$ 2NaOH(aq)+ H₂(g)+ Cl₂(g)

What is the proper cell diagram for the reaction 2AgCl(s)+ H₂(g) $\rightarrow$ 2Ag(s)+ 2H⁺(aq)+ 2Cl^-(aq)

Given: Ag⁺(aq)+ e^- $\rightarrow$ Ag(s) E° = 0.80 V Fe³⁺(aq)+ e^- $\rightarrow$ Fe²⁺(aq) E^$\circ$ = 0.77 V Cu²⁺(aq)+ 2e^- $\rightarrow$ Cu(s) E^$\circ$= 0.34 V Which is the strongest reducing agent?

If the standard potential for Cu²⁺(aq)/Cu⁺(aq)is 0.15 V and the standard potential for Cu²⁺(aq)/Cu(s)is 0.34 V,calculate the standard potential for Cu⁺(aq)+ e^- $\rightarrow$ Cu(s).

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)m Pb²⁺(aq)|Pb(s) Is +0.23 V at 25^$\circ$C.Calculate the equilibrium constant for the reaction of 1 M Pb²⁺(aq)with 1M SO₄²^-(aq).

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Exam 14: Electrochemistry

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H2(g) →\rightarrow→ 2Au(s)+ 2H+(aq)+ 2Cl-(aq)

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn2+/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,which half-reaction occurs in the left-hand cell compartment?

Of the following five ions or molecules,which is the strongest reducing agent?

Calculate E for the half-reaction below. 2H+(aq,1.00 * 10-5 M)+ 2- →\rightarrow→ H2(g,1.00 atm)

In a working electrochemical cell (+ cell voltage),the cations in the salt bridge move toward the cathode.

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn2+/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,what is the equation for the cell reaction?

When a sample of an unknown metal is dropped into 1 M H+(aq)under standard conditions,bubbles are observed.The unknown metal could be silver.

Which pair of metals will dissolve in nitric acid?

What reaction occurs at the cathode in the following cell diagram? Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l)

How many moles of O2(g)are produced by electrolysis of Na2SO4(aq)if 0.120 A is passed through the solution for 65.0 min?

The equilibrium constant for the reaction 2Hg(l)+ 2Cl-(aq)+ Ni2+(aq) →\rightarrow→ Ni(s)+ Hg2Cl2(s) Is 5.6 * 10-20 at 25 ∘\circ∘ C.Calculate the value of E ∘\circ∘ for a cell utilizing this reaction.

Consider the following cell: Pt|Fe2+(aq,0.50 M),Fe3+(aq,0.30 M)m Fe3+(aq,0.035 M),Fe2+(aq,0.010)|Pt The standard potential for the Fe3+/Fe2+ couple is +0.77 V.Calculate the cell voltage at 25 ∘\circ∘ C.

For the cell diagram Pt|H2(g)|H+(aq)mCo3+(aq),Co2+(aq)|Pt write the reaction that occurs at the cathode.

For the cell diagram Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l) What reaction occurs at the cathode?

How many moles of Cl2(g)are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,the "chloralkali" process,is 2NaCl(aq)+ 2H2O(l) →\rightarrow→ 2NaOH(aq)+ H2(g)+ Cl2(g)

What is the proper cell diagram for the reaction 2AgCl(s)+ H2(g) →\rightarrow→ 2Ag(s)+ 2H+(aq)+ 2Cl-(aq)

Given: Ag+(aq)+ e- →\rightarrow→ Ag(s) E° = 0.80 V Fe3+(aq)+ e- →\rightarrow→ Fe2+(aq) E ∘\circ∘ = 0.77 V Cu2+(aq)+ 2e- →\rightarrow→ Cu(s) E ∘\circ∘ = 0.34 V Which is the strongest reducing agent?

If the standard potential for Cu2+(aq)/Cu+(aq)is 0.15 V and the standard potential for Cu2+(aq)/Cu(s)is 0.34 V,calculate the standard potential for Cu+(aq)+ e- →\rightarrow→ Cu(s).

The standard potential of the cell Pb(s)|PbSO4(s)|SO42-(aq)m Pb2+(aq)|Pb(s) Is +0.23 V at 25 ∘\circ∘ C.Calculate the equilibrium constant for the reaction of 1 M Pb2+(aq)with 1M SO42-(aq).

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Chemical Equilibria

Acids and Bases

Aqueous Equilibria

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

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Write the proper cell diagram for the following reaction: 2AuCl(s)+ H₂(g) $\rightarrow$ 2Au(s)+ 2H⁺(aq)+ 2Cl^-(aq)

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn²⁺/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,which half-reaction occurs in the left-hand cell compartment?

Calculate E for the half-reaction below. 2H⁺(aq,1.00 * 10^-⁵ M)+ 2^- $\rightarrow$ H₂(g,1.00 atm)

Use the following diagram of a cell to answer questions -In the cell shown above,A is a standard Zn²⁺/Zn electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is -0.76 V,what is the equation for the cell reaction?

When a sample of an unknown metal is dropped into 1 M H⁺(aq)under standard conditions,bubbles are observed.The unknown metal could be silver.

What reaction occurs at the cathode in the following cell diagram? Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l)

How many moles of O₂(g)are produced by electrolysis of Na₂SO₄(aq)if 0.120 A is passed through the solution for 65.0 min?

The equilibrium constant for the reaction 2Hg(l)+ 2Cl^-(aq)+ Ni²⁺(aq) $\rightarrow$ Ni(s)+ Hg₂Cl₂(s) Is 5.6 * 10^-20 at 25^$\circ$C.Calculate the value of E^$\circ$ for a cell utilizing this reaction.

Consider the following cell: Pt|Fe²⁺(aq,0.50 M),Fe³⁺(aq,0.30 M)m Fe³⁺(aq,0.035 M),Fe²⁺(aq,0.010)|Pt The standard potential for the Fe³⁺/Fe²⁺ couple is +0.77 V.Calculate the cell voltage at 25^$\circ$C.

For the cell diagram Pt|H₂(g)|H⁺(aq)mCo³⁺(aq),Co²⁺(aq)|Pt write the reaction that occurs at the cathode.

For the cell diagram Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l) What reaction occurs at the cathode?

How many moles of Cl₂(g)are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,the "chloralkali" process,is 2NaCl(aq)+ 2H₂O(l) $\rightarrow$ 2NaOH(aq)+ H₂(g)+ Cl₂(g)

What is the proper cell diagram for the reaction 2AgCl(s)+ H₂(g) $\rightarrow$ 2Ag(s)+ 2H⁺(aq)+ 2Cl^-(aq)

Given: Ag⁺(aq)+ e^- $\rightarrow$ Ag(s) E° = 0.80 V Fe³⁺(aq)+ e^- $\rightarrow$ Fe²⁺(aq) E^$\circ$ = 0.77 V Cu²⁺(aq)+ 2e^- $\rightarrow$ Cu(s) E^$\circ$= 0.34 V Which is the strongest reducing agent?

If the standard potential for Cu²⁺(aq)/Cu⁺(aq)is 0.15 V and the standard potential for Cu²⁺(aq)/Cu(s)is 0.34 V,calculate the standard potential for Cu⁺(aq)+ e^- $\rightarrow$ Cu(s).

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)m Pb²⁺(aq)|Pb(s) Is +0.23 V at 25^$\circ$C.Calculate the equilibrium constant for the reaction of 1 M Pb²⁺(aq)with 1M SO₄²^-(aq).