Electrochemistry Test

Result

Electrochemistry Test - 6

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Weekly Quiz Competition

Question 1
1 / -0.25

Three Faradays of electricity are passed through molten Al₂ O₃ , aqueous solution of CuSO₄ and molten NaCl taken in three different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of-

A
1 mole : 2 mole : 3 mole

B
1 mole : 1.5 mole : 3 mole

C
3 mole : 2 mole : 1 mole

D
1 mole : 1.5 mole : 2 mole

Solution

gm equivalent of Al = gm eq. of Cu = gm eq. of Na
3 = 3 = 3
3/3/ = 3/2 = 1
1 : 1.5 : 3
Question 2
1 / -0.25

The quantity of electricity required to liberate 0.01g equivalent of an element at the electrode is-

A
9650C

B
96500C

C
965C

D
96.5C

Solution
Question 3
1 / -0.25

The unit of electrochemical equivalent is-

A
Gm ampere^-1

B
Gm/coulomb

C
Gm- ampere

D
Coulomb/gram

Solution

Z = w/it
w in gm
it in columb.
so z = gm/columb
Question 4
1 / -0.25

One faraday of electricity will liberate one mole of metal from a solution of-

A
AuCl₃

B
CuSO₄

C
BaCl₂

D
KCl

Solution

Since KCl has the n-factor of 1 so 1 faraday of electricity will liberate one mole of metal from a solution.
Question 5
1 / -0.25

The number of faraday required to generate 1 mole of Mg from MgCl₂ is-

A
1

B
2

C
3

D
4

Solution

Since magnesium has the n-factor 2 so the number of faraday rquired to genereate 1 mole of Mg will be 2 .
Question 6
1 / -0.25

One gm metal M⁺² was discharged by the passage of 1.81 ×10²² electrons. What is the atomic weight of metal?

A
33.35

B
133.4

C
66.7

D
55

Solution
Question 7
1 / -0.25

One mole of electron passes through each of the solution of AgNO₃ , CuSO₄ and AlCl₃ when Ag, Cu and Al are deposited at cathode. The molar ratio of Ag, Cu and Al deposited are

A
1 : 1 : 1

B
6 : 3 : 2

C
6 : 3 : 1

D
1 : 3 : 6

Solution

Molar ratio
All have the same equivalent
Question 8
1 / -0.25

Salts of A (atomic weight = 7), B (atomic weight = 27) and C (atomic weight = 48) were electrolysed under identical conditions using the same quantity of electricity. It was found that when 2.1 g of A was deposited, the weights of B and C deposited were 2.7 and 7.2 g. The valencies of A, B and C respectively are

A
3, 1 and 2

B
1, 3 and 2

C
3, 1 and 3

D
2, 3 and 2

Solution

If x = 1 ⇒y = 3, z = 2
Question 9
1 / -0.25

The density of Cu is 8.94 g cm^–3 . The quantity of electricity needed to plate an area 10 cm ×10cm to a thickness of 10^-2 cm using CuSO₄ solution would be

A
13586 C

B
27172 C

C
40758 C

D
20348 C

Solution

Volume : 10 ×10 ×10^–2 = 1 cm³
mass of Cu = 8.94 g

= 27172 C
Question 10
1 / -0.25

During electrolysis of an aqueous solution of sodium sulphate if 2.4 L of oxygen at STP was liberated at anode. The volume of hydrogen at STP, liberated at cathode would be :

A
1.2 L

B
2.4 L

C
2.6 L

D
4.8 L

Solution

Equivalent of H₂ = Equivalent of O₂

= 4.8 L