Strongest reducing agent among the following is
(i) $ {Na^+ + e^- ->Na_{(s)} \:\: E^{\circ} = - 2.71 \, V}$
(ii) $ {Al^{3+} + 3e^- ->Al_{(s)} \:\: E^{\circ} = - 1.66 \, V}$
(iii) $ {F_{2(g)} + 2e^- ->2F^- \:\: E^{\circ} = + 2.87 \, V}$
(iv) ${2H_2 O+ 2e^- ->H_{2(g)} + 2OH^-_{(aq)} \:\: E^{\circ} = - 0.83\, V}$
- iv
- iii
- ii
- i
The Correct Option is D
Solution and Explanation
The standard reduction potential affects the reducing agent's potency. The powerful nature of the reducing agent is shown by the large negative value.
Here, the fourth chemical reaction has the most lower E0 value so, it’ll be the strongest reducing agent.
A substance is a reducing agent when it loses electrons during a redox reaction and is oxidized to a higher valency state. A reducing agent is one of the reactants in an oxidation-reduction process; it decreases the other reactant by releasing electrons. If the reducing agent does not transfer electrons to other reactants in the reaction, the reduction process cannot occur.
Oxygen atoms are lost during reduction whereas electrons and hydrogen are obtained. Gaining oxygen while losing electrons and hydrogen is the process of oxidation. As a result, an element's oxidation state increases during oxidation, whereas it decreases during reduction.
A few characteristics of such reducing agents are–
- Electrons are often lost by reducing agents. Metals in the s-block of the periodic table are well-recognized for being effective reducers.
- The reducing agent oxidized after losing electrons, which led to the opposing reactant being reduced by receiving electrons.
- All effective reducing agents include species with low ionization energies as well as atoms with low electronegativity and a strong capacity of an atom or molecule to attract bonding electrons.
- All oxidation and reduction processes include the transfer of electrons.
- A material is considered to be reduced when it receives electrons and to be oxidized when it loses electrons.
- If a chemical has a significant propensity to lose electrons, it is referred to be a strong reducing agent.
Top Questions on Redox reactions
- Consider the following redox reaction:\[\text{MnO}_4^- + \text{H}^+ + \text{H}_2 \text{C}_2 \text{O}_4 \rightleftharpoons \text{Mn}^{2+} + \text{H}_2 \text{O} + \text{CO}_2\]The standard reduction potentials are given as below (E\(_\text{red}\)):\[E^\circ_{\text{MnO}_4^-/\text{Mn}^{2+}} = +1.51 \, \text{V}\]\[E^\circ_{\text{CO}_2/\text{H}_2 \text{C}_2 \text{O}_4} = -0.49 \, \text{V}\]If the equilibrium constant of the above reaction is given as \(K_\text{eq} = 10^x\), then the value of (x = ________ ) (nearest integer).
- JEE Main - 2024
- Chemistry
- Redox reactions
- Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A): In aqueous solutions \( \text{Cr}^{2+} \) is reducing while \( \text{Mn}^{3+} \) is oxidising in nature.
Reason (R): Extra stability to half-filled electronic configuration is observed than incompletely filled electronic configuration.
In the light of the above statement, choose the most appropriate answer from the options given below:- JEE Main - 2024
- Chemistry
- Redox reactions
- The number of ions from the following that have the ability to liberate hydrogen from a dilute acid is _______. Ti2+, Cr2+ and V2+.
- JEE Main - 2024
- Chemistry
- Redox reactions
- Only \( 2 \, \text{mL} \) of \( \text{KMnO}_4 \) solution of unknown molarity is required to reach the end point of a titration of \( 20 \, \text{mL} \) of oxalic acid (\( 2 \, \text{M} \)) in acidic medium. The molarity of \( \text{KMnO}_4 \) solution should be ______ \( \text{M} \).
- JEE Main - 2024
- Chemistry
- Redox reactions
- When \( \text{MnO}_2 \) and \( \text{H}_2\text{SO}_4 \) is added to a salt (A), the greenish yellow gas liberated as salt (A) is:
- JEE Main - 2024
- Chemistry
- Redox reactions
Questions Asked in COMEDK UGET exam
- A $2\,kg$ mass lying on a table is displaced in the horizontal direction through $50\,cm$. The work done by the normal reaction will be
- COMEDK UGET - 2015
- work, energy and power
- The numbers of $ {H^+}$ ions present in 1 mL of a solution whose pH is 13
- COMEDK UGET - 2015
- Equilibrium
- A mixture of methylamine and dimethylamine is given to you. The reagents used to separate the components of the mixture are
- $\cot^{-1} (21) + \cot^{-1} (13) + \cot^{-1} (-8) =$
- COMEDK UGET - 2015
- Inverse Trigonometric Functions
- Pick the incorrect statement among those given below.
- COMEDK UGET - 2015
- Chemical bonding and molecular structure
Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.
SUBSCRIBE TO OUR NEWS LETTER
