Question 1

A cell that uses bromine to oxidize chloride ion under standard conditions at 298 K has a positive potential.

Accepted Answer

The answer of A cell that uses bromine to oxidize...

Question 2

Which metal will dissolve in hydrochloric acid?

Accepted Answer

Fe (iron) will dissolve in hydrochloric acid, producing iron(II) chloride and hydrogen gas. Ag (silver), Pt (platinum), and Au (gold) are noble metals and do not easily dissolve in hydrochloric acid.

Question 3

Which species will reduce Br₂ but not V³⁺?

Accepted Answer

Copper (Cu) can reduce Br2 to Br- but cannot reduce V3+ to V2+ because its standard reduction potential is higher than that of V3+/V2+.

Question 4

A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

Accepted Answer

The given reaction represents the oxidation half-reaction, which involves the loss of electrons (e-). The standard reduction potential of this half-reaction is +1.08 V (at 298 K). Since the potential of an oxidation reaction is the negative of the reduction potential, the potential of the given reaction would be -1.08 V (under standard conditions). Therefore, the correct answer is option B, which is "false."

Question 5

If the standard potentials for the couples Cu²⁺/Cu, Ag⁺/Ag,And Fe²⁺/Fe are+0.34,+0.80,And -0.44 V,Respectively,Which is the strongest reducing agent?

Accepted Answer

The strongest reducing agent is the one with the most negative standard potential, which is Fe with a standard potential of -0.44 V.

Question 6

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Ag(s)|AgCl(s)|Cl^-(aq)M Cu²⁺(aq)|Cu(s) Is +0.12 V.What is the standard potential of the AgCl/Ag,Cl^- electrode?

Accepted Answer

The standard potential of the AgCl/Ag, Cl- electrode can be calculated using the given potentials of the Cu2+/Cu and the overall cell. The overall cell potential is the difference between the cathode and anode potentials. Given that the Cu2+/Cu potential is +0.34 V and the overall cell potential is +0.12 V, the potential of the AgCl/Ag, Cl- electrode can be found by rearranging the cell potential equation: E(cell) = E(cathode) - E(anode). Here, E(cell) = +0.12 V and E(cathode) = E(Cu2+/Cu) = +0.34 V. Solving for E(anode), which is the potential of the AgCl/Ag, Cl- electrode, gives E(anode) = E(cathode) - E(cell) = +0.34 V - +0.12 V = +0.22 V.

Question 7

Which species will reduce Ag⁺ but not Fe²⁺?

Accepted Answer

Hydrogen gas (H₂) can reduce Ag⁺ to Ag but does not have enough reducing power to reduce Fe²⁺ to Fe.

Question 8

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

Accepted Answer

The strongest reducing agent is the one with the lowest (most negative) standard reduction potential. Cu has the lowest reduction potential among the given options, making it the strongest reducing agent.

Question 9

Consider the reaction: 2Ag⁺(aq)+ Cu(s)$\rightarrow$Cu²⁺(aq)+ 2Ag(s)If the standard potentials of Ag⁺ and Cu²⁺ are +0.80 V and +0.34 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Accepted Answer

The answer of Consider the reaction: 2Ag⁺(aq)+ Cu(s)$\rightarrow$Cu²⁺(aq)+ 2Ag(s)If the standard...

Question 10

Which of the following is the strongest oxidizing agent?

Accepted Answer

The answer of Which of the following is the strongest...

Question 11

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

Accepted Answer

The strongest reducing agent is the one that is most easily oxidized, meaning it loses electrons most readily. Chromium in the +2 oxidation state (Cr^2+) is known to be a strong reducing agent because it has a high tendency to donate electrons to become more stable by achieving a more positive oxidation state.

Question 12

If the standard potentials for the couples Fe³⁺/Fe²⁺, MnO₄2^-,H⁺/Mn²⁺,H₂O,Zn²⁺/Zn,V³⁺/V²⁺,And Br₂/Br^- are +0.77,+1.51,-0.76,-0.26,And +1.09 V,Respectively,Which is the strongest oxidizing agent?

Accepted Answer

The strongest oxidizing agent is the one with the highest standard potential, which is +1.51 V for MnO4-/Mn2+.

Question 13

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

The observation of bubbles indicates a possible reaction with the acid. While some metals, such as magnesium or zinc, could react with the acid to produce bubbles, silver is a noble metal and would not react with the acid under standard conditions. Therefore, the unknown metal is not likely to be silver.

Question 14

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb²⁺(aq)M Cu²⁺(aq)|Cu(s) Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

Accepted Answer

The answer of The standard potential of the Cu²⁺/Cu electrode...

Question 15

Which of the following occurs when HNO₃(aq), Cu(s), And Pt(s)Are mixed under standard conditions?

Accepted Answer

Copper (Cu) reacts with nitric acid (HNO3) under standard conditions to dissolve and form copper nitrate, nitrogen dioxide, and water. Platinum (Pt) does not react with nitric acid under these conditions.

Question 16

Which pair of metals will dissolve in nitric acid?

Accepted Answer

Ag (Silver) and Fe (Iron) will dissolve in nitric acid. Pt (Platinum) and Au (Gold) are noble metals and are resistant to corrosion and oxidation in moist air, including resistance to nitric acid.

Question 17

Which of the following occurs when HCl(aq), Cu(s),And Fe(s)Are mixed under standard conditions?

Accepted Answer

Iron (Fe) is more reactive than copper (Cu) and will react with hydrochloric acid (HCl) to form iron chloride and hydrogen gas, causing the iron to dissolve. Copper does not react with HCl under standard conditions.

Question 18

Calculate E^$\omicron$ for the following cell. Zn(s)|Zn²⁺(aq)MCl^-(aq)|AgCl(s)|Ag(s)

Accepted Answer

First, we need to identify the half-reactions:
Oxidation: Zn(s) -> Zn2+(aq) + 2 e-
Reduction: 2 Ag+(aq) + 2 e- -> 2 Ag(s)

Next, we need to find the standard reduction potentials for each half-reaction:
Zn2+(aq) + 2 e- -> Zn(s)   E° = -0.76 V
2 Ag+(aq) + 2 e- -> 2 Ag(s)   E° = +0.80 V

Now, we can calculate the standard cell potential (E°cell) using the formula:
E°cell = E°reduction + (-E°oxidation)
E°cell = (+0.80 V) + (-(-0.76 V))
E°cell = +1.56 V

Since the given reaction is not at standard conditions (it includes concentrations of species), we need to use the Nernst equation to calculate the actual cell potential (Ecell):
Ecell = E°cell - (RT/nF) ln(Q)
where:
R = gas constant = 8.314 J/mol-K
T = temperature in Kelvin
n = number of electrons transferred in the balanced equation (2 in this case)
F = Faraday's constant = 96,485 C/mol
ln = natural logarithm
Q = reaction quotient

We are not given the temperature or concentrations of species, so we cannot calculate the actual cell potential (Ecell). However, we can determine that the correct answer choice is D (+0.98 V) because it is closest to the standard cell potential (E°cell = +1.56 V). This suggests that the reaction is likely to be spontaneous and have a positive Ecell under standard conditions.

Question 19

Consider the following reaction: 2Cu⁺(aq)$\rightarrow$ Cu(s)+ Cu²⁺(aq)If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Accepted Answer

The standard cell potential ($E^\circ_{cell}$) for the reaction is calculated using the formula: $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$. Given that the standard potentials for Cu^2+ + 2e^- → Cu(s) is +0.34 V and for Cu^+ + e^- → Cu(s) is +0.52 V, the reaction as written shows Cu^+ being oxidized to Cu^2+ and Cu being reduced from Cu^2+, making Cu^2+ the cathode and Cu^+ the anode. Therefore, $E^\circ_{cell} = 0.34 V - 0.52 V = -0.18 V$. However, the sign must be considered in the context of the reaction direction, and the correct interpretation leads to a positive value for the cell potential in the context of the given reaction, indicating a mistake in the sign interpretation. The correct calculation without considering sign inversion mistakenly suggests $E^\circ_{cell} = 0.18 V$, but the correct approach to calculate $E^\circ_{cell}$ should consider the actual roles of cathode and anode in the electrochemical series, leading to a reevaluation of the answer.

Question 20

Which species will oxidize Cr²⁺ but not Mn²⁺?

Accepted Answer

The answer of Which species will oxidize Cr²⁺ but not...

Quiz 6: Reactions

A cell that uses bromine to oxidize chloride ion under standard conditions at 298 K has a positive potential.

Which metal will dissolve in hydrochloric acid?

Which species will reduce Br₂ but not V³⁺?

A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

If the standard potentials for the couples Cu²⁺/Cu, Ag⁺/Ag,And Fe²⁺/Fe are+0.34,+0.80,And -0.44 V,Respectively,Which is the strongest reducing agent?

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Ag(s) |AgCl(s) |Cl^-(aq) M Cu²⁺(aq) |Cu(s) Is +0.12 V.What is the standard potential of the AgCl/Ag,Cl^- electrode?

Which species will reduce Ag⁺ but not Fe²⁺?

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

Consider the reaction: 2Ag⁺(aq) + Cu(s) $\rightarrow$ Cu²⁺(aq) + 2Ag(s) If the standard potentials of Ag⁺ and Cu²⁺ are +0.80 V and +0.34 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Which of the following is the strongest oxidizing agent?

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

If the standard potentials for the couples Fe³⁺/Fe²⁺, MnO₄2^-,H⁺/Mn²⁺,H₂O,Zn²⁺/Zn,V³⁺/V²⁺,And Br₂/Br^- are +0.77,+1.51,-0.76,-0.26,And +1.09 V,Respectively,Which is the strongest oxidizing agent?

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.

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s) |Pb²⁺(aq) M Cu²⁺(aq) |Cu(s) Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

Which of the following occurs when HNO₃(aq) , Cu(s) , And Pt(s) Are mixed under standard conditions?

Which pair of metals will dissolve in nitric acid?

Which of the following occurs when HCl(aq) , Cu(s) ,And Fe(s) Are mixed under standard conditions?

Calculate E^$\omicron$ for the following cell. Zn(s) |Zn²⁺(aq) MCl^-(aq) |AgCl(s) |Ag(s)

Consider the following reaction: 2Cu⁺(aq) $\rightarrow$ Cu(s) + Cu²⁺(aq) If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Which species will oxidize Cr²⁺ but not Mn²⁺?

Quiz 6: Reactions

A cell that uses bromine to oxidize chloride ion under standard conditions at 298 K has a positive potential.

Which metal will dissolve in hydrochloric acid?

Which species will reduce Br2 but not V3+?

A cell that uses bromine to oxidize hydrogen to H+ under standard conditions at 298 K has a negative potential?

If the standard potentials for the couples Cu2+/Cu, Ag+/Ag,And Fe2+/Fe are+0.34,+0.80,And -0.44 V,Respectively,Which is the strongest reducing agent?

The standard potential of the Cu2+/Cu electrode is +0.34 V and the standard potential of the cell Ag(s) |AgCl(s) |Cl-(aq) M Cu2+(aq) |Cu(s) Is +0.12 V.What is the standard potential of the AgCl/Ag,Cl- electrode?

Which species will reduce Ag+ but not Fe2+?

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

Consider the reaction: 2Ag+(aq) + Cu(s) →\rightarrow→ Cu2+(aq) + 2Ag(s) If the standard potentials of Ag+ and Cu2+ are +0.80 V and +0.34 V,Respectively,Calculate the value of E ο\omicronο for the given reaction.

Which of the following is the strongest oxidizing agent?

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

If the standard potentials for the couples Fe3+/Fe2+, MnO42-,H+/Mn2+,H2O,Zn2+/Zn,V3+/V2+,And Br2/Br- are +0.77,+1.51,-0.76,-0.26,And +1.09 V,Respectively,Which is the strongest oxidizing agent?

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.

The standard potential of the Cu2+/Cu electrode is +0.34 V and the standard potential of the cell Pb(s) |Pb2+(aq) M Cu2+(aq) |Cu(s) Is +0.47 V.What is the standard potential of the Pb2+/Pb electrode?

Which of the following occurs when HNO3(aq) , Cu(s) , And Pt(s) Are mixed under standard conditions?

Which pair of metals will dissolve in nitric acid?

Which of the following occurs when HCl(aq) , Cu(s) ,And Fe(s) Are mixed under standard conditions?

Calculate E ο\omicronο for the following cell. Zn(s) |Zn2+(aq) MCl-(aq) |AgCl(s) |Ag(s)

Consider the following reaction: 2Cu+(aq) →\rightarrow→ Cu(s) + Cu2+(aq) If the standard potentials of Cu2+ and Cu+ are +0.34 and +0.52 V,Respectively,Calculate the value of E ο\omicronο for the given reaction.

Which species will oxidize Cr2+ but not Mn2+?

Which species will reduce Br₂ but not V³⁺?

A cell that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K has a negative potential?

If the standard potentials for the couples Cu²⁺/Cu, Ag⁺/Ag,And Fe²⁺/Fe are+0.34,+0.80,And -0.44 V,Respectively,Which is the strongest reducing agent?

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Ag(s) |AgCl(s) |Cl^-(aq) M Cu²⁺(aq) |Cu(s) Is +0.12 V.What is the standard potential of the AgCl/Ag,Cl^- electrode?

Which species will reduce Ag⁺ but not Fe²⁺?

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

Consider the reaction: 2Ag⁺(aq) + Cu(s) $\rightarrow$ Cu²⁺(aq) + 2Ag(s) If the standard potentials of Ag⁺ and Cu²⁺ are +0.80 V and +0.34 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

If the standard potentials for the couples Fe³⁺/Fe²⁺, MnO₄2^-,H⁺/Mn²⁺,H₂O,Zn²⁺/Zn,V³⁺/V²⁺,And Br₂/Br^- are +0.77,+1.51,-0.76,-0.26,And +1.09 V,Respectively,Which is the strongest oxidizing agent?

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.

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s) |Pb²⁺(aq) M Cu²⁺(aq) |Cu(s) Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

Which of the following occurs when HNO₃(aq) , Cu(s) , And Pt(s) Are mixed under standard conditions?

Calculate E^$\omicron$ for the following cell. Zn(s) |Zn²⁺(aq) MCl^-(aq) |AgCl(s) |Ag(s)

Consider the following reaction: 2Cu⁺(aq) $\rightarrow$ Cu(s) + Cu²⁺(aq) If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Which species will oxidize Cr²⁺ but not Mn²⁺?