In the reaction- Zn-FeSO4-ZnSO4-Fe

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Valency and Oxidation State

In the reacti...

Question

In the reaction: $Zn + {FeSO}_{4} \to {ZnSO}_{4} + Fe$

$Zn$ gets oxidized.

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

$Fe$ gets oxidized.

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$Zn$ is an oxidizing agent.

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$Zn$ and $Fe$ are both oxidized.

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A
$Zn$ gets oxidized.

(A) $Zn$ gets oxidized is the correct option.
Redox reaction:
In a redox reaction or Oxidation-Reduction process, the oxidation and reduction reactions always happen simultaneously.
The substance getting reduced in a chemical reaction is known as the oxidizing agent, while a substance that is getting oxidized is known as the reducing agent.
Hence, in this reaction $Zn$ gets oxidized going from an oxidation state of $0$ to $+ 2$ , whereas $Fe$ gets reduced going from an oxidation state of $+ 2$ to $0$ .
The explanation of the incorrect option
(B) $Fe$ gets oxidized
$Fe$ gets reduced going from an oxidation state of $+ 2$ to $0$ .
(C) $Zn$ is an oxidizing agent
In this reaction $Zn$ gets oxidized so it acts as a reducing agent.
(D) $Zn$ and $Fe$ are both oxidized
$Zn$ gets oxidized but $Fe$ gets reduced.
Therefore, in the reaction: $Zn + {FeSO}_{4} \to {ZnSO}_{4} + Fe$ , $Zn$ gets oxidized and A is the correct option.

Suggest Corrections

Similar questions

Complete the following table

Element	Atomic number $(Z)$	Mass number $(A)$	Number of protons	Number of electrons $(e)$	Number of neutrons $(n)$
$F$

Given below are the end products of different reactions involving glucose.

Write the reaction number in front of the following:

(1) Anaerobic reaction =

(2) Reaction in human muscles =

(3) Aerobic respiration =

(4) Reaction in plant cells =

(5) Reaction in liver =

Consider the following reaction (unbalanced)

$Zn + H_{2} {SO}_{4} \to G + R + X (hot conc)$

$Zn + NaOH \to T + Q (conc)$

$G + H_{2} S + {NH}_{3} (aq) \to Z + X + Y$

Choose the correct option(s)

The standard electrode potential of two half cells is given below-

${Ni}^{2 +} + 2 e^{-} \to Ni$ ; $E_{1}^{0} = - 0.25 V$

${Zn}^{2 +} + 2 e^{-} \to Zn$ ; $E_{2}^{0} = - 0.77 V$

The voltage cell formed by combining the two half cells would be:

Consider a $70 %$ efficient hydrogen-oxygen cell working under the standard condition at $1$ bar and $298$ K. Its cell reaction is

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$

The work derived from the cell on the consumption of $1.0 \times 10^{- 3}$ $mol of H_{2} (g)$ is used to compress $1.00 mol$ of a monoatomic ideal gas in a thermally insulated container. What is the change in the temperature (in $K$ ) of the ideal gas?

The standard reduction potentials for the two half-cells are given below

$O_{2} (g) + 4 H^{+} (aq) + 4 e^{-} \to 2 H_{2} O (l)$ , $E^{0}$ = $1.23 V$

$2 H^{+} (aq) + 2 e^{-} \to H_{2} (g)$ , $E^{0}$ = $0.00 V$

Use $F = 96500 {Cmol}^{- 1}$ , $R = 8.314 {Jmol}^{- 1} K^{- 1}$ .

Join BYJU'S Learning Program

In the reaction: Zn+FeSO4→ZnSO4+Fe

In the reaction: $Zn + {FeSO}_{4} \to {ZnSO}_{4} + Fe$