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Exam 18: Electrochemistry

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Question 41

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Consider the galvanic cell shown below. -What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

A) +0.03 V
B) +0.02 V
C) -0.02 V
D) -0.03 V

E) A) and B)
F) None of the above

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Question 42

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What is the reduction half-reaction for the following overall cell reaction? Pb²⁺(aq) + 2 Ag(s) → Pb(s) + 2 Ag⁺(aq)

A) Ag(s) + e^- → Ag⁺(aq)
B) Ag⁺(aq) + e^- → Ag(s)
C) Pb²⁺(aq) + 2 e^- → Pb(s)
D) Pb²⁺(aq) + e^- → Pb(s)

E) C) and D)
F) B) and C)

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Question 43

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O₂(g) + 4 H⁺(aq) + 4 e^- → 2 H₂O(l) E° = +1.23 V Pb²⁺(aq) + 2 e^- → Pb(s) E° = -0.13 V 2 H₂O(l) + 2 e^- → H₂(g) + 2 OH^-(aq) E° = -0.83 V Based on the half-reactions above,electrolysis of an aqueous solution of Pb(NO₃) ₂ is expected to produce.

Consider the following galvanic cell. -What is the shorthand notation for the cell?

The standard potential for the following galvanic cell is +0.90 V: 3 Cu²⁺(aq) + 2 Ga(s) ⇌ 3 Cu(s) + 2 Ga³⁺(aq) Given that the standard reduction potential for the Cu²⁺/Cu half-cell is +0.34 V,what is the standard reduction potential for the Ga³⁺/Ga half-cell?

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 40.0 minutes?

Consider the galvanic cell shown below. -What is the shorthand notation for the cell?

NaNO₃(aq) is employed in the salt bridge.Give the direction of electron flow and the direction of ion flow from the salt bridge.

When suspected drunk drivers are tested with a Breathalyzer,the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: 3CH₃CH₂OH(aq) + 2Cr₂O₇^-2 (aq) + 16H⁺(aq) 3CH₃CO₂H(aq) + 4Cr⁺³(aq) + 11H₂O (l) If Eº for this cell is 1.30V and the standard half-cell potential of Cr₂O₇^-2(aq) to Cr⁺³ is 1.358 V,what is the standard half-cell reduction potential for the conversion of acetic acid to ethanol?

For the hypothetical reaction 3 A + 2 B^x → 3 A^y + 2 B,E° = 0.85 V and G° = -495 kJ.For this reaction the values of x and y are ________ and ________.

Consider the following table of standard reduction potentials: Which substance is the strongest reducing agent?

What is the oxidation half reaction in the following chemical reaction? Cr₂O₇^2-(aq) + 6 Cl^-(aq) + 14 H⁺(aq) → 2 Cr³⁺(aq) + 3 Cl₂(aq) + 7 H₂O(l)

For the galvanic cell Pt(s) ∣ Sn²⁺(aq) ,Sn⁴⁺(aq) ∣∣ Cd²⁺(aq) ∣ Cd(s) ,what is the function of the Pt(s) ?

Ag⁺(aq) + e^- → Ag(s) E° = +0.800 V AgBr(s) + e^- → Ag(s) + Br^-(aq) E° = +0.071 V Br₂(l) + 2 e^- → 2 Br^-(aq) E° = +1.066 V Use some of the data above to calculate K_sp at 25°C for AgBr.

In the shorthand notation for a galvanic cell,a single vertical line (|)represents a ________,and a double vertical line (|| )represents a ________.

How many moles of electrons,n,are transferred in the following reduction-oxidation reaction? 2 MnO₄^-(aq) + 16 H⁺(aq) + 10 Cl^-(aq) → 2 Mn²⁺(aq) + 5 Cl₂(g) + 8 H₂O(l)

A galvanic cell consists of one half-cell that contains Ag(s) and Ag⁺(aq) ,and one half-cell that contains Cu(s) and Cu²⁺(aq) .What species are produced at the electrodes under standard conditions? Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.34 V

What are the coefficients in front of NO₃^-(aq) and Mg(s) when the following redox equation is balanced in an acidic solution? ________ NO₃^-(aq) + ________ Mg(s) → ________ NO(g) + ________ Mg²⁺(aq)

What is the shorthand notation that represents the following galvanic cell reaction? Fe(s) + Cu(NO₃) ₂(aq) → Fe(NO₃) ₂(aq) + Cu(s)

Based on the half-reactions and their respective standard reduction potentials below,which addition to an aqueous solution containing Fe(NO₃) ₂ will result in a reaction under standard-state conditions? O₂(g) + 4 H⁺ +4 e^- → 2 H₂O(l) 1.23 V Fe³⁺(aq) + e^- → Fe²⁺(aq) 0.77 V Cu²⁺(aq) + 2 e^- → Cu(s) 0.34 V 2 H⁺(aq) + 2 e^- → H₂(g) 0.00 V Ni²⁺(aq) + + 2 e^- → Ni(s) -0.26 V Fe²⁺(aq) + 2 e^- → Fe(s) -0.45 V