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Exam 18: Electrochemistry

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Question 51

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C.(The equation is balanced.) $\quad$$\quad$ Pb(s) + Br₂(l) → Pb²⁺(aq) + 2 Br⁻(aq) Pb²⁺(aq) + 2 e^- → Pb(s) $\quad$$\quad$ E° = -0.13 V Br₂(l) + 2 e^- → 2 Br^- (aq) $\quad$$\quad$ E° = +1.07 V

A) +1.20 V
B) +0.94 V
C) -0.94 V
D) -1.20 V
E) -0.60 V

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Question 52

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$$\quad$$\quad$ Al(s) | Al³⁺(aq,0.115 mol L^-1) $\|$ Al³⁺(aq,3.89 mol L^-1) | Al(s) E°(Al³⁺/Al) = -1.66 V

A) +1.66 V
B) +0.060 V
C) 0.00 V
D) +0.090 V
E) +0.030 V

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Question 53

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What is undergoing oxidation in the redox reaction represented by the following cell notation? $\quad$$\quad$$\quad$ Fe(s) | Fe³⁺(aq) $\|$ Cl₂(g) | Cl^- (aq) | Pt(s)

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

The standard emf for the cell using the overall cell reaction below is +2.20 V: $\quad$$\quad$ 2Al(s) + $3 \mathrm { I } _ { 2 }$ (s) ? $2 \mathrm { AL } ^ { 3 + }$ (aq) + $6 \mathrm { I } ^ { - }$ (aq) The emf generated by the cell when [ $\mathrm { Al } ^ { 3 + }$ ] = 4.5 × $10 ^ { - 3 }$ mol L^-1 and [ $\mathrm { I } ^ { - }$ ] = 0.15 mol L^-1 is $\text { V. }$

What is the reaction at the cathode in a breathalyzer?

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? $\quad$$\quad$ Ag⁺ (aq) + e^- → Ag(s)

What is electrolysis?

What is the oxidizing agent in the redox reaction represented by the following cell notation? $\quad$$\quad$$\quad$ Sn(s) | Sn²⁺(aq) $\|$ Ag⁺(aq) | Ag(s)

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$$\quad$$\quad$ Sn(s) | Sn²⁺(aq,0.010 mol L^-1) $\|$ Ag⁺(aq,1.00 mol L^-1) | Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Describe how water can be made to be a good conductor of electrical current.

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ $\mathrm { Mg } ^ { 2 + }$ ] = 0.500 M and [ $\mathrm { Fe } ^ { 3 + }$ ] = 2.00 M $\quad$$\quad$ Mg(s) + $\mathrm { Fe } ^ { 3 + }$ (aq) ? $\mathrm { Mg } ^ { 2 + }$ (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Which of the following metals will dissolve in HCl?

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

A galvanic cell consists of a Zn²⁺/Zn half-cell and a standard hydrogen electrode.If the Zn²⁺/Zn half-cell standard cell functions as the anode,and the standard cell potential is 0.76 V,what is the standard reduction potential for the Zn²⁺/Zn half-cell?

Which of the following is the strongest reducing agent?

Determine the redox reaction represented by the following cell notation: $\quad$$\quad$ Mg(s) | Mg²⁺(aq) $\|$ Cu²⁺(aq) | Cu(s)

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? $\quad$$\quad$$\quad$ Ni(s) | Ni²⁺(aq) || Cl₂(g) | Cl^-(aq) | C(s)