FiltersDone

Question type

Essay

Multiple Choice

Short Answer

True False

Matching

Exam 18: Electrochemistry

Show Answer

Share

---

All types

Filters

Study Flashcards

Question 51

Multiple Choice

Review LaterAdd Note

Review Later

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)

A) Fe(s)
B) Fe³⁺(aq)
C) Cl₂(g)
D) Cl^- (aq)
E) Pt(s)

Correct Answer

verified

Show Answer

Question 52

Essay

Review LaterAdd Note

Review Later

What is electrolysis?

Correct Answer

verified

An electrical curren...

View Answer

Show Answer

Question 53

Multiple Choice

Review LaterAdd Note

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

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

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?

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

Which of the following is the strongest reducing agent?

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

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

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

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)

What is the reaction at the cathode in a breathalyzer?

Which of the following metals will dissolve in HCl?

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?

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)

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

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)