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Exam 20: Principles of Reactivity: Electron Transfer Reactions

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Question 1

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Write a balanced chemical equation for the overall reaction represented by the cell notation below.Mn(s) | Mn²⁺(aq) || Zn²⁺(aq) | Zn(s)

A) 2Mn(s) + Zn²⁺(aq) $\to$ Zn(s) + 2Mn²⁺(aq)
B) Mn(s) + Mn²⁺(aq) $\to$ Zn(s) + Zn²⁺(aq)
C) Mn(s) + Zn²⁺(aq) $\to$ Zn(s) + Mn²⁺(aq)
D) 2Zn(s) + Mn²⁺(aq) $\to$ Mn(s) + 2Zn²⁺(aq)
E) Zn(s) + Mn²⁺(aq) $\to$ Mn(s) + Zn²⁺(aq)

F) B) and C)
G) A) and B)

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Question 2

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What is the standard cell potential ( ) for the following below, 2Ag(s) + Pb²⁺(aq) $\to$ 2Ag⁺(aq) + Pb(s) Given the following standard reduction potentials. Ag⁺(aq) + e^- $\to$ Ag(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ =0.8 V Pb²⁺(aq) +2e^- $\to$ Pb(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ =-0.126 V

A) -0.926 V
B) 0.926 V
C) -1.726 V
D) 1.726 V
E) 1.474 V

F) D) and E)
G) C) and E)

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Question 3

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Calculate E°_cell for the cell for the reaction below, 2Cr(s) + 3Sn⁴⁺(aq) $\to$ 3Sn²⁺(aq) +2Cr³⁺(aq) Given the following standard reduction potentials. Cr³⁺(aq) + 3e^- $\to$ Cr(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = -0.74 V Sn⁴⁺(aq) + 2e^- $\to$ Sn²⁺(aq) $~~~~~~~~$$~ ~~$ E ^$\circ$ = 0.15V

Al³⁺ is reduced to Al(s) at an electrode.If a current of 2.75 ampere is passed for 36 hours,what mass of aluminum is deposited at the electrode? Assume 100% current efficiency.

Which of the following statements is/are CORRECT? 1) A nickel-cadmium battery is an example of a secondary or rechargeable battery,often used in rechargeable cordless appliances. 2) Hydrogen-oxygen fuel cells use the heat of combustion of hydrogen to recharge lead storage batteries. 3) LeClanché cells are the most efficient rechargeable batteries,but they are rarely used due their high cost of production.

Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used aboard NASA's space shuttles.

For the cell reaction l ) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

In the following electrochemical cell,what is the reduction half reaction? Cu(s) | Cu²⁺(aq) || Fe³⁺(aq) ,Fe²⁺(aq) | Pt(s)

Calculate E_cell for the following electrochemical cell at 25°C given that the standard cell potential, E°_cell,is 0.460 V. Cu(s) | Cu²⁺(aq,0.012 M) || Ag⁺(aq,0.17 M) | Ag(s)

An SHE electrode has been assigned a standard reduction potential,E ^$\circ$ ,of 0.00 Volts.Which reaction occurs at this electrode?

Calculate for the electrochemical cell below, Ag(s) | AgCl(s) | Cl^-(aq,1.0 M) || Cu²⁺(aq,1.0 M) | Cu(s) Given the following standard reduction potentials. Cu²⁺(aq) + 2 e^- $\to$ Cu(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +0.337 V AgCl(s) + e^- $\to$ Ag(s) + Cl^-(aq) $~~~~~~~~$ E ^$\circ$ = +0.222 V

Explain the function of a salt bridge in a voltaic cell.

Given the following two half-reactions,write the overall reaction in the direction in which it is spontaneous and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- $\to$ Pb(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = -0.126 V Fe³⁺(aq) + e^- $\to$ Fe²⁺(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +0.771 V

The use of electrical energy to produce chemical change is known as ________.An example of this process is the reduction of NaCl( )to produce Na(s).

What is the correct cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Pb⁴⁺(aq) + 2e^- Pb²⁺(aq) .

What is the correct cell notation for a voltaic cell based on the reaction below? Cu²⁺(aq) + Fe(s) $\to$ Cu(s) + Fe²⁺(aq)

Consider the following half-reactions: Cl₂(g) + 2 e^- $\to$ 2 Cl^-(aq) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +1.36 V Ag⁺(aq) + e^- $\to$ Ag(s) $~~~ ~~~~$$~~~~ ~~~$$~~ ~~~~$ E ^$\circ$ = +0.80 V Cu²⁺(aq) + 2 e^- $\to$ Cu(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +0.34 V Sn²⁺(aq) + 2 e^- $\to$ Sn(s) $~~~~~ ~$$~~~ ~$$~~~~~~~~$ E ^$\circ$ = -0.14 V Al³⁺(aq) + 3 e^- $\to$ Al(s) $~~~~~~~~$$~~~ ~~~~$$~~~$ E ^$\circ$ = -1.66 V Which of the above elements or ions will reduce Cu²⁺(aq) ?

Which of the following are standard conditions for an electrochemical cell? 1) Solutes in aqueous solution has a concentration of 1 M. 2) Gaseous reactants or products have a pressure of 1 bar. 3) Solids are present in quantities of 1 mole.

The unit for electromotive force,emf,is the Volt.A Volt is equal to

The following reaction occurs spontaneously. 2 Fe(s) + 3 Cl₂(aq) $\to$ 2 Fe³⁺(aq) + 6 Cl^-(aq) Write the balanced oxidation half-reaction.