(A) The standard reduction potential of $Zn^{2+}/Zn$ is $-0.76 \ V$,while that of $Fe^{2+}/Fe$ is $-0.44 \ V$.Since zinc has a more negative electrode

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(A) The standard reduction potential of $Zn^{2+}/Zn$ is $-0.76 \ V$,while that of $Fe^{2+}/Fe$ is $-0.44 \ V$.Since zinc has a more negative electrode potential than iron,it acts as a sacrificial anode.Zinc gets oxidized in preference to iron,thereby protecting the iron from rusting.Thus,both the Assertion and the Reason are correct,and the Reason is the correct explanation of the Assertion.

Class 12 Chemistry Electrochemistry Electrochemical cells

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Assertion : Galvanised iron does not rust.
Reason : Zinc has a more negative electrode potential than iron.

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A
If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
B
If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
C
If the Assertion is correct but Reason is incorrect.
D
If both the Assertion and Reason are incorrect.

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Upon dipping a copper rod into an aqueous solution of the salt,the solution that turns blue is

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Which of the following is $NOT$ a difficulty in setting up a Standard Hydrogen Electrode $(SHE)$?

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$A$ galvanic cell has an electrical potential of $1.1 \ V$. If an opposing potential of $1.1 \ V$ is applied to this cell,what will happen to the cell reaction and the current flowing through the cell?

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Give the symbolic representation of the following galvanic cells:
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Assertion : Galvanised iron does not rust.Reason : Zinc has a more negative electrode potential than iron.

Similar Questions

Upon dipping a copper rod into an aqueous solution of the salt,the solution that turns blue is

In which of the following solutions will a blue color appear after some time when a piece of $Cu$ metal is added?

Which of the following is $NOT$ a difficulty in setting up a Standard Hydrogen Electrode $(SHE)$?

$A$ galvanic cell has an electrical potential of $1.1 \ V$. If an opposing potential of $1.1 \ V$ is applied to this cell,what will happen to the cell reaction and the current flowing through the cell?

Give the symbolic representation of the following galvanic cells:$(i)$ Daniell cell$(ii)$ Copper-Silver cell

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Assertion : Galvanised iron does not rust.
Reason : Zinc has a more negative electrode potential than iron.

Give the symbolic representation of the following galvanic cells:
$(i)$ Daniell cell
$(ii)$ Copper-Silver cell