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CHXI08:REDOX REACTIONS

315390 Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
$E^{\circ} v a l u e s : F e^{3 +} / F e^{2 +} = + 0 . 77;$
$I_{2} / I^{-} = + 0 . 54;$
$C u^{2 +} / C u = + 0 . 34;$
$A g^{+} / A g = + 0 . 80 V$

1

{Fe}^{3 +}

and

I^{-}

2

{Ag}^{+}

and

Cu

3

{Fe}^{3 +}

and

Cu

4

Ag

and

{Fe}^{3 +}

CHXI08:REDOX REACTIONS

315391 Assertion :
Lithium ion is a poor oxidising agent.
Reason :
Lithium ion has the lowest electrode potential.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In electrochemical series lithium ion is placed at the bottom with a lowest reduction potential of $- 3.04 V$ . This means it is stable in its oxidised state and is a poor oxiding agent. So the option (1) is correct.

CHXI08:REDOX REACTIONS

315392 Consider the following statement(s)
(A) Iron reacts with dilute $H_{2} {SO}_{4}$ to evolve $H_{2} (g)$ but $Ag$ does not
(B) Copper dissolves in dilute ${HNO}_{3}$ but not in dilute $HCl$ .
(C) Amongst the halogens, fluorine is the best oxidant because it is the most known as electronegative element
Choose the correct statement(s)

1 A & B

2 B & C

3 A & C

4 A, B & C

Explanation:

Iron releases $H_{2}$ gas from $H_{2} {SO}_{4}$ as it is above $H^{+}$ in electrochemical series.
Copper is less electropositive metal.
Fluorine is the best oxident due to its high reduction potential.

CHXI08:REDOX REACTIONS

315393 Which reaction is not feasible?

1

2 KI + {Br}_{2} \to 2 KBr + I_{2}

2

2 KBr + I_{2} \to 2 KI + {Br}_{2}

3

2 KBr + {Cl}_{2} \to 2 KCl + {Br}_{2}

4

2 H_{2} O + 2 F_{2} \to 4 HF + O_{2}

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315394 Which of the following reaction will not take place?

1

Fe + H_{2} {SO}_{4} \to {FeSO}_{4} + H_{2}

2

Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag

3

2 KBr + I_{2} \to 2 KI + {Br}_{2}

4

CuO + H_{2} \to Cu + H_{2} O

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315390 Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
$E^{\circ} v a l u e s : F e^{3 +} / F e^{2 +} = + 0 . 77;$
$I_{2} / I^{-} = + 0 . 54;$
$C u^{2 +} / C u = + 0 . 34;$
$A g^{+} / A g = + 0 . 80 V$

1

{Fe}^{3 +}

and

I^{-}

2

{Ag}^{+}

and

Cu

3

{Fe}^{3 +}

and

Cu

4

Ag

and

{Fe}^{3 +}

CHXI08:REDOX REACTIONS

315391 Assertion :
Lithium ion is a poor oxidising agent.
Reason :
Lithium ion has the lowest electrode potential.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In electrochemical series lithium ion is placed at the bottom with a lowest reduction potential of $- 3.04 V$ . This means it is stable in its oxidised state and is a poor oxiding agent. So the option (1) is correct.

CHXI08:REDOX REACTIONS

315392 Consider the following statement(s)
(A) Iron reacts with dilute $H_{2} {SO}_{4}$ to evolve $H_{2} (g)$ but $Ag$ does not
(B) Copper dissolves in dilute ${HNO}_{3}$ but not in dilute $HCl$ .
(C) Amongst the halogens, fluorine is the best oxidant because it is the most known as electronegative element
Choose the correct statement(s)

1 A & B

2 B & C

3 A & C

4 A, B & C

Explanation:

Iron releases $H_{2}$ gas from $H_{2} {SO}_{4}$ as it is above $H^{+}$ in electrochemical series.
Copper is less electropositive metal.
Fluorine is the best oxident due to its high reduction potential.

CHXI08:REDOX REACTIONS

315393 Which reaction is not feasible?

1

2 KI + {Br}_{2} \to 2 KBr + I_{2}

2

2 KBr + I_{2} \to 2 KI + {Br}_{2}

3

2 KBr + {Cl}_{2} \to 2 KCl + {Br}_{2}

4

2 H_{2} O + 2 F_{2} \to 4 HF + O_{2}

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315394 Which of the following reaction will not take place?

1

Fe + H_{2} {SO}_{4} \to {FeSO}_{4} + H_{2}

2

Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag

3

2 KBr + I_{2} \to 2 KI + {Br}_{2}

4

CuO + H_{2} \to Cu + H_{2} O

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315390 Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
$E^{\circ} v a l u e s : F e^{3 +} / F e^{2 +} = + 0 . 77;$
$I_{2} / I^{-} = + 0 . 54;$
$C u^{2 +} / C u = + 0 . 34;$
$A g^{+} / A g = + 0 . 80 V$

1

{Fe}^{3 +}

and

I^{-}

2

{Ag}^{+}

and

Cu

3

{Fe}^{3 +}

and

Cu

4

Ag

and

{Fe}^{3 +}

CHXI08:REDOX REACTIONS

315391 Assertion :
Lithium ion is a poor oxidising agent.
Reason :
Lithium ion has the lowest electrode potential.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In electrochemical series lithium ion is placed at the bottom with a lowest reduction potential of $- 3.04 V$ . This means it is stable in its oxidised state and is a poor oxiding agent. So the option (1) is correct.

CHXI08:REDOX REACTIONS

315392 Consider the following statement(s)
(A) Iron reacts with dilute $H_{2} {SO}_{4}$ to evolve $H_{2} (g)$ but $Ag$ does not
(B) Copper dissolves in dilute ${HNO}_{3}$ but not in dilute $HCl$ .
(C) Amongst the halogens, fluorine is the best oxidant because it is the most known as electronegative element
Choose the correct statement(s)

1 A & B

2 B & C

3 A & C

4 A, B & C

Explanation:

Iron releases $H_{2}$ gas from $H_{2} {SO}_{4}$ as it is above $H^{+}$ in electrochemical series.
Copper is less electropositive metal.
Fluorine is the best oxident due to its high reduction potential.

CHXI08:REDOX REACTIONS

315393 Which reaction is not feasible?

1

2 KI + {Br}_{2} \to 2 KBr + I_{2}

2

2 KBr + I_{2} \to 2 KI + {Br}_{2}

3

2 KBr + {Cl}_{2} \to 2 KCl + {Br}_{2}

4

2 H_{2} O + 2 F_{2} \to 4 HF + O_{2}

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315394 Which of the following reaction will not take place?

1

Fe + H_{2} {SO}_{4} \to {FeSO}_{4} + H_{2}

2

Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag

3

2 KBr + I_{2} \to 2 KI + {Br}_{2}

4

CuO + H_{2} \to Cu + H_{2} O

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315390 Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
$E^{\circ} v a l u e s : F e^{3 +} / F e^{2 +} = + 0 . 77;$
$I_{2} / I^{-} = + 0 . 54;$
$C u^{2 +} / C u = + 0 . 34;$
$A g^{+} / A g = + 0 . 80 V$

1

{Fe}^{3 +}

and

I^{-}

2

{Ag}^{+}

and

Cu

3

{Fe}^{3 +}

and

Cu

4

Ag

and

{Fe}^{3 +}

CHXI08:REDOX REACTIONS

315391 Assertion :
Lithium ion is a poor oxidising agent.
Reason :
Lithium ion has the lowest electrode potential.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In electrochemical series lithium ion is placed at the bottom with a lowest reduction potential of $- 3.04 V$ . This means it is stable in its oxidised state and is a poor oxiding agent. So the option (1) is correct.

CHXI08:REDOX REACTIONS

315392 Consider the following statement(s)
(A) Iron reacts with dilute $H_{2} {SO}_{4}$ to evolve $H_{2} (g)$ but $Ag$ does not
(B) Copper dissolves in dilute ${HNO}_{3}$ but not in dilute $HCl$ .
(C) Amongst the halogens, fluorine is the best oxidant because it is the most known as electronegative element
Choose the correct statement(s)

1 A & B

2 B & C

3 A & C

4 A, B & C

Explanation:

Iron releases $H_{2}$ gas from $H_{2} {SO}_{4}$ as it is above $H^{+}$ in electrochemical series.
Copper is less electropositive metal.
Fluorine is the best oxident due to its high reduction potential.

CHXI08:REDOX REACTIONS

315393 Which reaction is not feasible?

1

2 KI + {Br}_{2} \to 2 KBr + I_{2}

2

2 KBr + I_{2} \to 2 KI + {Br}_{2}

3

2 KBr + {Cl}_{2} \to 2 KCl + {Br}_{2}

4

2 H_{2} O + 2 F_{2} \to 4 HF + O_{2}

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315394 Which of the following reaction will not take place?

1

Fe + H_{2} {SO}_{4} \to {FeSO}_{4} + H_{2}

2

Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag

3

2 KBr + I_{2} \to 2 KI + {Br}_{2}

4

CuO + H_{2} \to Cu + H_{2} O

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315390 Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
$E^{\circ} v a l u e s : F e^{3 +} / F e^{2 +} = + 0 . 77;$
$I_{2} / I^{-} = + 0 . 54;$
$C u^{2 +} / C u = + 0 . 34;$
$A g^{+} / A g = + 0 . 80 V$

1

{Fe}^{3 +}

and

I^{-}

2

{Ag}^{+}

and

Cu

3

{Fe}^{3 +}

and

Cu

4

Ag

and

{Fe}^{3 +}

CHXI08:REDOX REACTIONS

315391 Assertion :
Lithium ion is a poor oxidising agent.
Reason :
Lithium ion has the lowest electrode potential.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In electrochemical series lithium ion is placed at the bottom with a lowest reduction potential of $- 3.04 V$ . This means it is stable in its oxidised state and is a poor oxiding agent. So the option (1) is correct.

CHXI08:REDOX REACTIONS

315392 Consider the following statement(s)
(A) Iron reacts with dilute $H_{2} {SO}_{4}$ to evolve $H_{2} (g)$ but $Ag$ does not
(B) Copper dissolves in dilute ${HNO}_{3}$ but not in dilute $HCl$ .
(C) Amongst the halogens, fluorine is the best oxidant because it is the most known as electronegative element
Choose the correct statement(s)

1 A & B

2 B & C

3 A & C

4 A, B & C

Explanation:

Iron releases $H_{2}$ gas from $H_{2} {SO}_{4}$ as it is above $H^{+}$ in electrochemical series.
Copper is less electropositive metal.
Fluorine is the best oxident due to its high reduction potential.

CHXI08:REDOX REACTIONS

315393 Which reaction is not feasible?

1

2 KI + {Br}_{2} \to 2 KBr + I_{2}

2

2 KBr + I_{2} \to 2 KI + {Br}_{2}

3

2 KBr + {Cl}_{2} \to 2 KCl + {Br}_{2}

4

2 H_{2} O + 2 F_{2} \to 4 HF + O_{2}

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .

CHXI08:REDOX REACTIONS

315394 Which of the following reaction will not take place?

1

Fe + H_{2} {SO}_{4} \to {FeSO}_{4} + H_{2}

2

Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag

3

2 KBr + I_{2} \to 2 KI + {Br}_{2}

4

CuO + H_{2} \to Cu + H_{2} O

Explanation:

$E_{I_{2} / I^{-}}^{0} = + 0.54 V; E_{B r_{2} / B r^{-}}^{0} = + 1.09 V$
${Br}_{2}$ is strong oxidant than $I_{2}$ . So, $I_{2}$ cannot displace bromine from $KBr$ .