Electrochemistry Test

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Electrochemistry Test - 30

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Weekly Quiz Competition

Question 1
1 / -0

How much electricity must pass through acidulated water to release $$22, 400\, cm^3$$ of hydrogen at N.T.P.?

A
96500 C

B
193000 C

C
22.4 C

D
95.5 C

Solution

We know that $$22,400cm^3$$ of $$H_2$$ means $$1$$ mole of $$H_2$$.

Now, we know that $$2H^{+}+2e^-\rightarrow H_2$$

Hence, for production of 1 mole of $$H_2$$, two moles of $$e^-$$ are required.

And, one mole of $$e^-$$ constitutes $$96500C$$

Hence, charge or electricity required$$=96500\times 2=193000C$$

Answer-(B)
Question 2
1 / -0

Rusting of iron is a chemical reaction. The reaction can be termed as:

A
combination reaction

B
addition reaction

C
both (A) and (B)

D
decomposition

Solution

Rusting of iron is a combination reaction. It occurs as follows-
$$Fe + H_2O + O_2 \rightarrow Fe_2O_3 xH_2O$$
Question 3
1 / -0

A solution of sodium chloride discharges $$6.1 \times 10^{16} Na^+$$ ions and $$4.6 \times 10^{16} Cl^-$$ ions in 10 seconds. Find the current passing through the solution.

A
1.7 mA

B
1.8 mA

C
1.9 mA

D
1.6 mA

Solution
Question 4
1 / -0

A voltaic cell converts:

A
electrical energy into chemical energy

B
chemical energy into electrical energy

C
light energy into electrical energy

D
mechanical energy into electrical energy

Solution

A voltaic cell also known as galvanic cell is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half cells. Chemical energy is converted to electrical energy.
Question 5
1 / -0

How many electrons constitute current of one micro ampere in one second?

A
$$6.25\times10^8$$

B
$$6.25\times10^{12}$$

C
$$6.25\times10^9$$

D
$$6.25\times10^{15}$$

Solution

Given: Current ,$$ I = 1\mu A = 10^{-6}A$$
We know that $$Q = ne, t = 1s$$
Where $$n$$ is the number of electrons and e is the charge on $$1$$ electron and $$e = 1.6\times10^{-19}C$$

$$n = \displaystyle\frac{I}{e} = \displaystyle\frac{10^{-6}}{1.6\times10^{-19}} = 6.25\times10^{12} Electrons$$
Question 6
1 / -0

Which of the following statements is true ?

A
Electrolysis is one of the applications of chemical effects of current

B
A metal wire shows chemical effect when a current is passed through it

C
Like charges attract each other

D
Charge flows only through negative charge carriers

Solution

Electrolysis is a method of using direct electric current to drive a chemical reaction. It involves the interchange of atoms and ions by the removal or addition of electrons.
Question 7
1 / -0

The weights of various ions liberated by passing the same current through different electrolytes are in the ratio of their:

A
Atomic weights

B
Equivalent weights

C
Molecular weights

D
Atomic numbers

Solution

The weights of various ions liberated by passing the same current through different electrolytes are in the ratio of their Equivalent weights.
So answer is B.
Question 8
1 / -0

$$1$$ faraday $$= \ ?$$

A
$$10000\ C$$

B
$$95000\ C$$

C
$$96.5 \ C$$

D
$$96500\ C$$

Solution

The Faraday constant, denoted by the symbol $$F$$ and named after Michael Faraday, is the magnitude of electric charge per mole of electrons. It has the accepted value $$96485.34$$ coulombs in round figure $$96500$$ coulombs.
Question 9
1 / -0

For purification of impure metals by the process of electrolysis

A
Salt solution of the impure metal is taken as an electrolyte

B
Salt solution of that metal in pure form is taken as an electrolyte

C
That metal in pure form is made as anode

D
Both $$(1)$$ and $$(3)$$

Solution

When an impure metal is purified using electrolytic refining impure metal is used as anode and pure metal is used as cathode and the salt solution of same metal in pure form that is being purified is taken as electrolyte.
Therefore, B is correct option.
Question 10
1 / -0

During electroplating by electrolysis, the article to be electroplated is:

A
Kept immersed in the electrolyte at the bottom.

B
Made the cathode of an electrolytic cell.

C
Made the anode of an electrolytic cell.

D
Made the electrolyte of the electrolytic cell.

Solution

During electroplating by electrolysis, the article to be electroplated as made the cathode of an electrolytic cell .

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Electrochemistry Test - 30

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Electrochemistry Test - 30

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Question 1

96500 C

193000 C

22.4 C

95.5 C

Solution

Question 2

combination reaction

addition reaction

both (A) and (B)

decomposition

Solution

Question 3

1.7 mA

1.8 mA

1.9 mA

1.6 mA

Solution

Question 4

electrical energy into chemical energy

chemical energy into electrical energy

light energy into electrical energy

mechanical energy into electrical energy

Solution

Question 5

$$6.25\times10^8$$

$$6.25\times10^{12}$$

$$6.25\times10^9$$

$$6.25\times10^{15}$$

Solution

Question 6

Electrolysis is one of the applications of chemical effects of current

A metal wire shows chemical effect when a current is passed through it

Like charges attract each other

Charge flows only through negative charge carriers

Solution

Question 7

Atomic weights

Equivalent weights

Molecular weights

Atomic numbers

Solution

Question 8

$$10000\ C$$

$$95000\ C$$

$$96.5 \ C$$

$$96500\ C$$

Solution

Question 9

Salt solution of the impure metal is taken as an electrolyte

Salt solution of that metal in pure form is taken as an electrolyte

That metal in pure form is made as anode

Both $$(1)$$ and $$(3)$$

Solution

Question 10

Kept immersed in the electrolyte at the bottom.

Made the cathode of an electrolytic cell.

Made the anode of an electrolytic cell.

Made the electrolyte of the electrolytic cell.

Solution

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