Free Printable Electroanalytical Quiz

1.

Calculate the cell potential for a galvanic cell with a zinc electrode at -0.76 V and a copper electrode at +0.34 V.

a)

0.34 V

b)

-1.10 V

c)

1.10 V

d)

0.58 V

2.

Which of the following is incorrect

a)

ΔG=-nFE

b)

E_cell =E_cathode-E_anode

c)

$E_{cell}=E^0-\frac{RT}{nF}\ln K$

d)

$\Delta G=nF\left(\frac{\partial E}{\partial T}\right)_P$

3.

Which of the following is an example for electrolytic process?

a)

Fuel Cell

b)

Battery undergoing discharging

c)

Battery undergoing charging

d)

Corrosion of iron in ambient conditions

4.

In the reaction, $2FeCl_3+H_2S\ \rightarrow\ 2FeCl_2+2HCl+S$

a)

FeCl₃acts an an oxidizing agent

b)

Both H₂S and FeCl₃ are oxidized

c)

FeCl₃ is oxidised while H₂S is reduced

d)

H₂S acts as an oxidizing agent

5.

If the oxidation potential of A/A⁺ and B/B⁺ are +2.37 V and +1.66 V respectively, in a spontaneous chemical reaction,

a)

A⁺ will be reduced by B

b)

A will reduce B⁺

c)

A will not reduce B⁺

d)

A and B will not reduce the oxidized forms of each other

6.

Which among the following is the strongest reducing agent (All standard potentials are w.r.t SHE)?

Given, $Fe^{2+}+2e^-\ \rightarrow\ Fe\ \left(-0.44V\right)$ ;

$Ni^{2+}+2e^-\ \rightarrow\ Ni\ \left(-0.25\ V\right)$ ;

$Sn^{2+}+2e^-\ \rightarrow\ Sn\ \left(-0.14\ V\right)$ ;;

$Zn^{2+}+2e^-\ \rightarrow\ Zn\ \left(-0.77V\right)$

a)

Fe

b)

Zn

c)

Ni

d)

Sn

7.

A process is said to be spontaneous if

a)

$\Delta G$ is negative

b)

$\Delta G$ is positive

c)

$\Delta S$ is negative

d)

$\Delta H$ is negative

8.

Which of the following is the correct Nernst equation?

a)

$E_{cell}=E_{cell}^0-\frac{RT}{nF}\log\left(\frac{\left[Ox\right]}{\left[Red\right]}\right)$

b)

$E_{cell}=E_{cell}^0-\frac{RT}{nF}\log\left(\frac{\left[Red\right]}{\left[Ox\right]}\right)$

c)

$E_{cell}=E_{cell}^0-\frac{RT}{nF}\ln\left(\frac{\left[Ox\right]}{\left[Red\right]}\right)$

d)

$E_{cell}=E_{cell}^0-\frac{RT}{nF}\ln\left(\frac{\left[Red\right]}{\left[Ox\right]}\right)$

9.

For the electrochemical cell, Mg(s)|Mg²⁺(aq, 1M)||Cu²⁺ (aq, 1M) | Cu(s) the standard emf of

the cell is 2.70 V at 300 K. When the concentration of Mg²⁺ is changed to x M, the cell

potential changes to 2.67 V at 300 K. The value of x is____.

a)

5

b)

4.5

c)

10

d)

2

10.

Reorder the following in the decreasing tendency to get reduced

a)

F

b)

Cl

c)

H⁺

d)

Al³⁺

e)

Li⁺

1)

2)

3)

4)

5)

11.

Calculate the potential of Cl^- concentration cell given below which uses sparingly soluble salt MCl.

M(s), MCl(s) | Cl^-_{(0.01 M)}||Cl^-_{(1 M)}| MCl(s), M(s)

a)

0.118 V

b)

-0.118 V

c)

0.059

d)

-0.059

12.

ΔG of the reaction $10H_2+5O_2\rightarrow10H_2O$ Given the E_cell = 1.23 V. Assume the Faraday constant as 96500 C and report your answer in kJ.

a)

-2374

b)

-237.4

c)

-1187

d)

-474.6

13.

The amount of Al electrodeposited at the cathode when 1 Faraday of Charge is passed through a solution containing 1 M Al(NO)₃

a)

9g

b)

18g

c)

0g

d)

27g

14.

In a Daniel cell, when operating in the galvanic mode, the overpotential at the zinc electrode/electrolyte interface is:

a)

>0

b)

<0

c)

=0

d)

Cannot be predicted

15.

If the standard potential of Zn²⁺/Zn redox couple is -0.76 V, what would be the value of potential when the concentration of Zn²⁺ is 0.01 M?

a)

-0.73

b)

-0.82

c)

0.73

d)

0.701

16.

Two hydrogen electrodes were combined to make a cell. If the partial pressures of hydrogen are 1 and 0.01 atm, respectively, the cell potential would be:

a)

RT/2F

b)

2.3RT/2F

c)

RT/F

d)

2.3RT/F

17.

For a hydrogen electrode, if the concentration of the H⁺ ions in the solution is increased, the potential would:

a)

Decrease

b)

Increase

c)

Remains constant

d)

Unpredictable

18.

The redox potential of H⁺/H₂ and O₂/H₂O couples are 0 V Vs SHE and 1.29 V vs (Hydrogen electrode operating with 0.1 M H⁺), respectively. If so, the minimum absolute voltage required for the electrolysis of water is about:

a)

1.23

b)

1.29

c)

2.0

d)

1.0

19.

If the potential of an electrode-electrolyte interface w.r.t. Ag/AgCl is -1.78 V in an electrolyte of pH = 6.8. The electrode’s potential w.r.t to hydrogen eectrode at that pH (6.8) is (Potential of Ag/AgCl,Cl^- reference w.r.t SHE is 0.197 V)

a)

-1.18 V

b)

-1.98 V

c)

1.18 V

d)

1.98 V

20.

Calculate the Redox potential of the following reaction in galvanic mode: $\text{BrO}_3^- + 3\text{H}_2\text{O} + 5e^- \rightleftharpoons 0.5\text{Br}_2 + 6\text{OH}^-$ If the emf of $\text{BrO}_3^-/\text{BrO}^-$ redox couple is 0.54 V vs. SHE and $\text{BrO}^-/\text{Br}_2$ redox couple is 0.45 V vs. SHE. Also calculate the quantity of electricity required in faradays to produce 1 mol of $\text{Br}_2$ from $\text{BrO}_3^-$ .

a)

0.522 V, 10

b)

2.61 V, 5

c)

1.05 V, 1

d)

0.261 V, 10

Electroanalytical Quiz

Total questions: 20

Worksheet time: 25mins

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