Free Printable Nernst Equation and Introduction to Electolysis

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Nernst Equation and Introduction to Electolysis

Total questions: 24

Worksheet time: 6hrs 0mins

Name

Class

Date

Which statement correctly describes the 2 electrodes?

The anode is negative and the cathode is positive

The anode and cathode are both positive

The anode is positive and the cathode is negative

The anode and cathode are both negative.

Explain why the electrolyte has to be a liquid.

So the ions can move

So the electrons can move

So that it doesn't get too hot

So the fish are ok

It is essetial that the electrolyte is a liquid so that...

Charged ions can migrate towards the electrodes.

The solution can move around.

The current can flow through it.

none of these

When NaCl solution is electrolysed what has forms at the anode?

Hydrogen

Oxygen

Chlorine

Sodium

What is the equation to show what happens to Cl ions at the anode.

Cl^- --> Cl + e-

2Cl^- --> Cl₂ + 2e-

Cl₂ + 2e-2Cl^-

Cl₂ + 2e-_-->2Cl^-

What state must the ionic compound be in to be electrolysed?

aqueous only

solid only

solid or aqueous only

molten or aqueous only

In an aqueous solution of copper chloride, which ions are attracted to the negative electrode?

Cu²⁺and Cl^-and H⁺and OH^-

Cu²⁺and H⁺

Cl^-and OH^-

Cu²⁺

What is the product formed at the cathode during the electrolysis of molten magnesium fluoride?

magnesium

hydrogen

fluorine

oxygen

What is the gas produced at the anode during the electrolysis of dilute hydrochloric acid?

water

oxygen

hydrogen

chlorine

10.

Choose the half-equation that shows the discharge of aluminium ion.

Al³⁺ - 3e^- --> Al

Al²⁺ + 3e^- --> Al

Al³⁺ + 3e^- --> Al

Al³⁺ --> Al + 3e^-

11.

What factors do not affect the products of electrolysis in the electrolysis of aqueous magnesium chloride using graphite electrodes?

position of ions in the electrochemical series

concentration of ions in the solution

type of electrodes

12.

What would be the product at the negative electrode in the electrolysis of Sodium Chloride solution

Sodium

Chlorine

Hydrogen

Oxygen

13.

What are the electrode products when molten silver iodide is electrolysed between inert electrodes?

14.

What particle carries the charge in the wire?

electron

proton

ion

atom

15.

Molten lead(II) bromide is electrolysed as shown.

16.

Using the Nernst Equation, calculate for the cell potential at standard temperature;

2Ag⁺(aq) [0.50 M] + Ni (s) ---> 2Ag (s) + Ni²⁺(aq) [0.20 M]

---

Ni (s) ---> Ni²⁺(aq) [0.20 M] +2e^- = E^o_red = -0.25 V

Ag⁺(aq) [0.50 M] + e^- ---> Ag (s) = E^o_red = +0.799 V

---

Answer with 4 sig figs, Values and UNIT

(a)

17.

A concentration cell consists of two Ag/Ag half-cells. In half-cell A, electrode A dips into 0.010 M AgNO₃; in half-cell B, electrode B dips into 4.0x10^-4 M AgNO₃ . What is the cell potential at 298.15 K? (with n=1) (Answer with Unit V, answer using decimal numbers, with 3 sig figs) e.g. 4.15 V

(a)

18.

Given half-cell equation; Cu²⁺ (aq) +2e $\rightarrow$ Cu (s)

Determine the amount of electricity charge required to produced 0.1 mol of Cu?

192,970 C

4825 C

482500 C

193000 C

None of these

19.

Given half-cell equation; Cu²⁺ (aq) +2e $\rightarrow$ Cu (s)

Determine the amount of electricity charge required to produced 0.1 mol of Cu?

19300 C

4825 C

482500 C

193000 C

20.

Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s)

E_CELL=E⁰_CELL-0.0591/6 log[Mg2+]³/[Al3+]²

E_CELL=E⁰_CELL-0.0591/6 log[Al3+]²/[Mg2+]³

E_CELL=E⁰_CELL+0.0591/3 log[Mg2+]³/[Al3+]²

E_CELL=E⁰_CELL-0.0591/3 log[Mg2+] /[Al3+]

21.

The concentration of sulfuric acid used in car-battery is more than 1.00 moldm^-3 and hence the condition becomes non-standard. The standard cell potential measured under standard conditions was found to be 1.60V. What would be the range of cell potential under non-standard conditions.

a) same as 1.60 V

b) less than 1.60 V

c) -1.60 V to +1.60 V

d) Around 2.0V

22.

Nernst equation for an electrode is based on the variation of electrode potential of an electrode with

Temperature

Concentration of electrolyte

Both a & b

Density of the electrodes

23.

For the cell reaction
2Al(s) + 3Mn2+(aq) → 2Al3+(aq) + 3Mn(s) at non-standard conditions. Predict whether Ecell is larger or smaller than E°cell:
[Al3+ ] = 2.0 M, [Mn2+ ] = 1.0 M

smaller

larger

the same

24.

For the cell reaction
2Al(s) + 3Mn2+(aq) → 2Al3+(aq) + 3Mn(s) at non-standard conditions. Predict whether Ecell is larger or smaller than E°cell:
[Al3+ ] = 1.0 M, [Mn2+] = 1.0 M