QBManager

ELECTROCHEMISTRY

19805 On passing the current in water voltameter, the hydrogen

1 Liberated at anode

2 Liberated at cathode

3 Does not liberate

4 Remains in the solution

Explanation:

(b) Because $H$ has positive charge.

ELECTROCHEMISTRY

19806 For depositing $1 g m$ of $C u$ in copper voltameter on passing $2 a m p e r e s$ of current, the time required will be (For copper $Z = 0.00033 g m / C$ )

1 Approx.

20

minutes

2 Approx.

25

minutes

3 Approx.

30

minutes

4 Approx.

35

minutes

Explanation:

(b) $m = Z i t$ $\Rightarrow$ $1 = 0.00033 \times 2 \times t$
$t = \frac{1}{0.00066 \times 60} m i n$ $= \frac{100000}{3960} \approx 25 m i n$

ELECTROCHEMISTRY

19807 According to Faraday's laws of electrolysis, the amount of decomposition is proportional to

1

\frac{1}{T i m e f o r w h i c h c u r e n t p a s s e s}

2 Electrochemical equivalent of the substance

3

\frac{1}{C u r r e n t}

4

\frac{1}{E l e c t r o c h e m i c a l e q u i v a l e n t}

Explanation:

The amount of decomposition (i.e., mass of the substance liberated during electrolysis) is proportional to electro chemical equivalent of the substance. Using the relation $[m = Z * i * t]$
where $Z$ is its electrochemical equivalent, $i$ is current, $t$ is time and $m$ is the mass deposited or liberated.
One can say that the amount of mass deposited will be proportional to the electrochemical equivalent of the substance.

ELECTROCHEMISTRY

19860 An electric current is passed through an aqueous solution of the following. Which one shall decompose

1 Urea

2 Glucose

3

A g N O_{3}

4 Ethyl alcohol

Explanation:

(c) $A g N O_{3}$ is an electrolyte.

ELECTROCHEMISTRY

19805 On passing the current in water voltameter, the hydrogen

1 Liberated at anode

2 Liberated at cathode

3 Does not liberate

4 Remains in the solution

Explanation:

(b) Because $H$ has positive charge.

ELECTROCHEMISTRY

19806 For depositing $1 g m$ of $C u$ in copper voltameter on passing $2 a m p e r e s$ of current, the time required will be (For copper $Z = 0.00033 g m / C$ )

1 Approx.

20

minutes

2 Approx.

25

minutes

3 Approx.

30

minutes

4 Approx.

35

minutes

Explanation:

(b) $m = Z i t$ $\Rightarrow$ $1 = 0.00033 \times 2 \times t$
$t = \frac{1}{0.00066 \times 60} m i n$ $= \frac{100000}{3960} \approx 25 m i n$

ELECTROCHEMISTRY

19807 According to Faraday's laws of electrolysis, the amount of decomposition is proportional to

1

\frac{1}{T i m e f o r w h i c h c u r e n t p a s s e s}

2 Electrochemical equivalent of the substance

3

\frac{1}{C u r r e n t}

4

\frac{1}{E l e c t r o c h e m i c a l e q u i v a l e n t}

Explanation:

The amount of decomposition (i.e., mass of the substance liberated during electrolysis) is proportional to electro chemical equivalent of the substance. Using the relation $[m = Z * i * t]$
where $Z$ is its electrochemical equivalent, $i$ is current, $t$ is time and $m$ is the mass deposited or liberated.
One can say that the amount of mass deposited will be proportional to the electrochemical equivalent of the substance.

ELECTROCHEMISTRY

19860 An electric current is passed through an aqueous solution of the following. Which one shall decompose

1 Urea

2 Glucose

3

A g N O_{3}

4 Ethyl alcohol

Explanation:

(c) $A g N O_{3}$ is an electrolyte.

ELECTROCHEMISTRY

19805 On passing the current in water voltameter, the hydrogen

1 Liberated at anode

2 Liberated at cathode

3 Does not liberate

4 Remains in the solution

Explanation:

(b) Because $H$ has positive charge.

ELECTROCHEMISTRY

19806 For depositing $1 g m$ of $C u$ in copper voltameter on passing $2 a m p e r e s$ of current, the time required will be (For copper $Z = 0.00033 g m / C$ )

1 Approx.

20

minutes

2 Approx.

25

minutes

3 Approx.

30

minutes

4 Approx.

35

minutes

Explanation:

(b) $m = Z i t$ $\Rightarrow$ $1 = 0.00033 \times 2 \times t$
$t = \frac{1}{0.00066 \times 60} m i n$ $= \frac{100000}{3960} \approx 25 m i n$

ELECTROCHEMISTRY

19807 According to Faraday's laws of electrolysis, the amount of decomposition is proportional to

1

\frac{1}{T i m e f o r w h i c h c u r e n t p a s s e s}

2 Electrochemical equivalent of the substance

3

\frac{1}{C u r r e n t}

4

\frac{1}{E l e c t r o c h e m i c a l e q u i v a l e n t}

Explanation:

The amount of decomposition (i.e., mass of the substance liberated during electrolysis) is proportional to electro chemical equivalent of the substance. Using the relation $[m = Z * i * t]$
where $Z$ is its electrochemical equivalent, $i$ is current, $t$ is time and $m$ is the mass deposited or liberated.
One can say that the amount of mass deposited will be proportional to the electrochemical equivalent of the substance.

ELECTROCHEMISTRY

19860 An electric current is passed through an aqueous solution of the following. Which one shall decompose

1 Urea

2 Glucose

3

A g N O_{3}

4 Ethyl alcohol

Explanation:

(c) $A g N O_{3}$ is an electrolyte.

ELECTROCHEMISTRY

19805 On passing the current in water voltameter, the hydrogen

1 Liberated at anode

2 Liberated at cathode

3 Does not liberate

4 Remains in the solution

Explanation:

(b) Because $H$ has positive charge.

ELECTROCHEMISTRY

19806 For depositing $1 g m$ of $C u$ in copper voltameter on passing $2 a m p e r e s$ of current, the time required will be (For copper $Z = 0.00033 g m / C$ )

1 Approx.

20

minutes

2 Approx.

25

minutes

3 Approx.

30

minutes

4 Approx.

35

minutes

Explanation:

(b) $m = Z i t$ $\Rightarrow$ $1 = 0.00033 \times 2 \times t$
$t = \frac{1}{0.00066 \times 60} m i n$ $= \frac{100000}{3960} \approx 25 m i n$

ELECTROCHEMISTRY

19807 According to Faraday's laws of electrolysis, the amount of decomposition is proportional to

1

\frac{1}{T i m e f o r w h i c h c u r e n t p a s s e s}

2 Electrochemical equivalent of the substance

3

\frac{1}{C u r r e n t}

4

\frac{1}{E l e c t r o c h e m i c a l e q u i v a l e n t}

Explanation:

The amount of decomposition (i.e., mass of the substance liberated during electrolysis) is proportional to electro chemical equivalent of the substance. Using the relation $[m = Z * i * t]$
where $Z$ is its electrochemical equivalent, $i$ is current, $t$ is time and $m$ is the mass deposited or liberated.
One can say that the amount of mass deposited will be proportional to the electrochemical equivalent of the substance.

ELECTROCHEMISTRY

19860 An electric current is passed through an aqueous solution of the following. Which one shall decompose

1 Urea

2 Glucose

3

A g N O_{3}

4 Ethyl alcohol

Explanation:

(c) $A g N O_{3}$ is an electrolyte.