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Redox Reactions

Ascorbic acid...

Question

Ascorbic acid $(C_{6} H_{8} O_{6})$ is a common antioxidant that protects our bodies against radicals. In the redox equation below that occurs in our stomach, which of the following pairs identifies the reducing and oxidizing agents respectively?
$C_{6} H_{8} O_{6} + 2 H^{+} + 2 N O_{2}^{-} \to C_{6} H_{6} O_{6} + 2 H_{2} O + 2 N O$

C_{6} H_{8} O_{6} a n d N O_{2}^{-}

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N O_{2}^{-} a n d C_{6} H_{8} O_{6}

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H^{+} a n d N O_{2}^{-}

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C_{6} H_{8} O_{6} a n d H^{+}

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Solution

The correct option is A $C_{6} H_{8} O_{6} a n d N O_{2}^{-}$
The given redox reaction is $C_{6} H_{8} O_{6} + 2 H^{+} + 2 N O_{2}^{-} \to C_{6} H_{6} O_{6} + 2 H_{2} O + 2 N O$ .
$H^{+}$ remains in the same oxidation state on both sides of equation, so it is neither the oxidizing nor reducing agent.

A species which can oxidised other and reduced itself in a redox reaction is called as oxidising agent.
Nitrite $(N O_{2}^{-})$ gets converted into nitric oxide $(N O)$ . Nitrogen is getting reduced because it is gaining electrons or losing bonds to oxygen, so $N O_{2}^{-}$ is the oxidizing agent.

A species which looses electron in a redox reaction is called as oxidising agent.
$C_{6} H_{8} O_{6},$ ascorbic acid, gets converted to $C_{6} H_{6} O_{6},$ dehydroascorbic acid. $C_{6} H_{8} O_{6}$ is getting oxidized since there is loss of electrons or loss of hydrogens, so it is the reducing agent.

$C_{6} H_{8} O_{6}$ and $N O_{2}^{-}$ in this order is the correct answer.

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Similar questions

Q. Ascorbic acid

(C_{6} H_{8} O_{6})

is a common antioxidant that protects our bodies against radicals. In the redox equation below that occurs in our stomach, which of the following pairs identifies the reducing and oxidizing agents respectively?

C_{6} H_{8} O_{6} + 2 H^{+} + 2 N O_{2}^{-} \to C_{6} H_{6} O_{6} + 2 H_{2} O + 2 N O

Q. The bones that protect the portion of the body below our stomach are called ________ .

Calculate the mass of ascorbic acid (Vitamin C, C₆H₈O₆) to be dissolved in
75 g of acetic acid to lower its melting point by 1.5°C. K_f = 3.9 K kg mol⁻¹.

Q. In which of the following equations.

H_{2} O_{2}

acts as a reducing agent in the acidic medium?

Electrochemical Battery

An electrochemical battery is a device powered by oxidation and reduction reactions that are physically separated. So that the electrons must travel through a wire from the reducing agent to the oxidizing agent.

The reducing agent loses electrons and is oxidized in a reaction that takes place at an electrode is called the anode. The oxidizing agent gains electrons and is reduced in a reaction that takes at an electrode is called the cathode.

To maintain a net zero charge in each compartment, there is a limited flow of ions through a salt bridge.

For example, in a car battery the reducing agent is oxidized by the following reaction, which involves a lead (

P b

) anode and sulfuric acid (

H_{2} S O_{4}

). Lead sulfate (

P b S O_{4}

), protons (

H

), and electrons (

e^{-}

) are produced.

At the cathode, the below reaction occurs :

P b O_{2} + H_{2} S O_{4} + 2 H^{+} + 2 e^{-} \to

PbSO_4+2H_2O$

At the anode, the below reaction occurs :

P b + H_{2} S O_{4} \to P b S O_{4} + 2 H^{+} + 2 e^{-}

Electrons are produced by a chemical reaction that takes place at the:

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Redox Reactions

Standard XIII Chemistry

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Ascorbic acid (C6H8O6) is a common antioxidant that protects our bodies against radicals. In the redox equation below that occurs in our stomach, which of the following pairs identifies the reducing and oxidizing agents respectively? C6H8O6+2H++2NO−2→C6H6O6+2H2O+2NO