Which is correct for a redox reaction where the standard electrode potential is negative?

ΔG^Θ = −nFE^Θ and ΔG^Θ = −RT ln K

A.   ΔG^Θ is negative and K is less than 1.

B.   ΔG^Θ is negative and K is greater than 1.

C.   ΔG^Θ is positive and K is less than 1.

D.   ΔG^Θ is positive and K is greater than 1.

Which signs for both E^θ_cell and ΔG^θ result in a spontaneous redox reaction occurring under standard conditions?

An iron rod is electroplated with silver. Which is a correct condition for this process?

A. The silver electrode is the positive electrode.

B. The iron rod is the positive electrode.

C. The electrolyte is iron(II) sulfate.

D. Oxidation occurs at the negative electrode.

Which statement is correct for the overall reaction in a voltaic cell?

2AgNO₃(aq) + Ni(s) → 2Ag(s) + Ni(NO₃)₂(aq)         E ^θ= +1.06 V

A.     Electrons flow from Ag electrode to Ni electrode.

B.     Ni is oxidized to Ni²⁺ at the cathode (negative electrode).

C.     Ag⁺ is reduced to Ag at the anode (positive electrode).

D.     Ag has a more positive standard electrode potential value than Ni.

Which statement is correct when a zinc spoon is electroplated with silver?

A.  The cathode (negative electrode) is made of silver.

B.  The anode (positive electrode) is the zinc spoon.

C.  The anode (positive electrode) is made of silver.

D.  The electrolyte is zinc sulfate solution.

What are the products when concentrated aqueous copper (II) chloride is electrolysed using platinum electrodes?

What would be the electrode potential, E^⦵, of the Mn²⁺(aq)|Mn (s) half-cell if Fe³⁺(aq)|Fe²⁺(aq) is used as the reference standard?

Mn²⁺ (aq) + 2e⁻ $\rightleftharpoons$ Mn (s)           E^⦵ = −1.18 V

Fe³⁺ (aq) + e⁻ $\rightleftharpoons$ Fe²⁺(aq)          E^⦵ = +0.77 V

A.  −1.95 V

B.  −0.41 V

C.  +0.41 V

D.  +1.95 V

Which gives the equation and cell potential of the spontaneous reaction?

What are the major products of electrolysing concentrated aqueous potassium iodide, KI(aq)?

What does not affect the mass of products formed in electrolysis of an aqueous solution?

A.     Current

B.     Duration of electrolysis

C.     Initial mass of cathode

D.     Charge on the ions

Consider the following standard electrode potentials:

Which species will react with each other spontaneously under standard conditions?

A.  Zn²⁺(aq) + Pb (s)

B.  Pb²⁺(aq) + Br₂(l)

C.  Zn (s) + Br⁻(aq)

D.  Pb (s) + Br₂ (l)

What are the products when dilute aqueous copper (II) nitrate is electrolysed using platinum electrodes?

E^⦵ (Cu | Cu²⁺) = –0.34 V.

Consider the following table of standard electrode potentials.

Which is the strongest oxidizing agent?

A. Pb²⁺

B. Pb

C. Al³⁺

D. Al

Which factors affect the amount of product formed at the cathode during electrolysis of molten salts?

    I. current
    II. time
    III. charge on the cation

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Three cells with platinum electrodes are connected in series to a DC power supply.

What is the ratio of moles formed at each cathode (negative electrode)?

Which conditions deposit the greatest mass of copper when solutions containing copper ions are electrolysed for 10 minutes?

Which combination would electroplate an object with copper?

What are the products when an aqueous solution of copper(II) sulfate is electrolysed using inert graphite electrodes?

Consider the standard electrode potentials:

Cr³⁺ (aq) + 3e⁻ $\rightleftharpoons$ Cr (s)       E^Θ = −0.74 V

Hg²⁺ (aq) + 2e⁻ $\rightleftharpoons$ Hg (l)      E^Θ = +0.85 V

What is the cell potential, in V, for the voltaic cell?

2Cr (s) + 3Hg²⁺ (aq) → 3Hg (l) + 2Cr³⁺ (aq)

A.   −1.59

B.   +0.11

C.   +1.07

D.   +1.59

What are the products of electrolysis when concentrated calcium bromide solution is electrolysed using graphite electrodes?

Which E^⦵ value, in V, for the reaction Mn (s) + Zn²⁺(aq) → Mn²⁺(aq) + Zn (s) can be deduced from the following equations?

Mn (s) + 2Ag⁺(aq) → Mn²⁺(aq) + 2Ag (s)     E^⦵ = 1.98 V

Zn (s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu (s)        E^⦵ = 1.10 V

Cu (s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag (s)      E^⦵ = 0.46 V

A.  0.42

B.  1.34

C.  2.62

D.  3.54

What is the order of increasing mass deposited by this electrolytic cell?

A_r  Ag = 108,  Cu = 64,  Sb = 122

A.  Ag < Cu < Sb

B.  Sb < Ag < Cu

C.  Cu < Ag < Sb

D.  Cu < Sb < Ag

What are the products when concentrated KBr (aq) is electrolyzed?

In the electrolysis of aqueous potassium nitrate, KNO₃(aq), using inert electrodes, 0.1 mol of a gas was formed at the cathode (negative electrode).

Which is correct?

What are the relative volumes of gas given off at E and F during electrolysis of the two cells in series? Assume all electrodes are inert.

A.     1:1

B.     1:2

C.     2:1

D.     5:2

Which is not a requirement of the standard hydrogen electrode (SHE)?

A. V = 1 dm³

B. p(H₂) = 100 kPa

C. use of platinum as the electrode material

D. [H₃O⁺] = 1 mol dm⁻³

What is the standard half-cell potential of copper if the “zero potential reference electrode” is changed from the standard hydrogen electrode to a standard zinc electrode?

A.     –1.1

B.     –0.34

C.     +0.34

D.     +1.1

In the electrolysis apparatus shown, 0.59 g of Ni is deposited on the cathode of the first cell.

What is the mass of Ag deposited on the cathode of the second cell?

A.  0.54 g

B.  0.59 g

C.  1.08 g

D.  2.16 g

Two cells undergoing electrolysis are connected in series.

If $x$ g of silver are deposited in cell 1, what volume of oxygen, in dm³ at STP, is given off in cell 2?

A_r(Ag) = 108; Molar volume of an ideal gas at STP = 22.7 dm³ mol⁻¹

A.    $\frac{x}{108}\times \frac{1}{4}\times 22.7$

B.    $\frac{x}{108}\times 4\times 22.7$

C.    $\frac{x}{108}\times \frac{1}{2}\times 22.7$

D.    $\frac{x}{108}\times 2\times 22.7$

Which aqueous solutions produce oxygen gas during electrolysis?

I.   Dilute CuCl₂(aq) with inert electrodes
II.  Dilute FeSO₄(aq) with inert electrodes
III. Dilute CuCl₂(aq) with copper electrodes

The standard electrode potentials are provided in the table:

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

What happens to the mass of each copper electrode when aqueous copper(II) sulfate solution is electrolysed?