Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 49

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A certain current passed through ${CuSO}_{4}$ solution for $100 seconds$ deposits $0.3175 g$ of copper. The current passed (in $A$ ) is:

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Important Questions on Electrochemistry

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 50

The salt that can be used in the salt bridge of an electrochemical cell is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 51

The conductometric titration curve (of conductance vs

mL

of

NaOH)

obtained when acetic acid is titrated against

NaOH

is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 52

In an alkaline energy cell the overall cell reaction is as follows:

$Zn (s) + 2 {MnO}_{2} (s) + 2 H_{2} O \to Zn {(OH)}_{2} (s) + 2 MnO (OH)$

Which of the following reactions is taking place at the cathode?

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 53

What is the charge on an ion of tin if

7.42 g

of metallic tin is deposited by passage of

24125 C

through a solution containing the ion?

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 55

The mass of the copper, in grams, deposited during the passage of

2.5 ampere

current through a

Cu (II)

sulphate solution for

1 hour

is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 57

Rusting of iron is due to the formation of:

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 59

The voltage for the cell:

Fe / {Fe}^{2 +} (0.001 M) / / {Cu}^{2 +} (0.10 M) / {Cu}^{2 +} (0.10 M) / {Cu}^{2 +} (0.10 M) / Cu

is

0.807 V

at

25 ° C

. What is the value of

E °

?

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Alpha Question Bank for Engineering: Chemistry>Chapter 9 - Electrochemistry>Exercise-4>Q 60

A current of

2.0 A

is used to plate

Ni (s)

from

500 mL

of a

1.0 {MNi}^{2 +}

[{Ni}^{2 +}]

after

3.0

hours?