`p_(4)(s)+3OH^(-)(aq)` . For this reaction the oxidizing and reducing agents are, respectively :

In the reaction ClO_(3)^(-)(aq)+5Cl^(-)(aq)+6H^(+)(aq)rarr3Cl_(2)(g)+3H_(2)O(l) the oxidizing and reducing agents are , respectively :

Explain oxidation, reduction, oxidising agent and reducing agent ?

In SO_2 an oxidizing agent or reducing agent or both?

P_(4)(s) + 3OH^(-) (aq) + 3H_(2)O (I) rarr PH_(3) (g) + 3H_(2)PO_(2)^(-) (aq) In the above equation, the species getting oxidized and reduced respectively are

Differentiate between an oxidizing agent and a reducing agent.

In photosynthetic bacteria, reaction centre and reducing agent are _______ and _______ respectively :-

Determining the realtive strengths of oxidizing and reducing agents a. Arrange the following oxidizing agents in order of increasing strength unde standard-state conditions: Br_(2)(1), Fe^(3+)(aq.), Cr_(2)O_(7)^(2-)(aq.) b. Arrange the following reducine agents in order of increasing strength under standard state condition: Al(a), Na(s), Zn(s) Strategy: Pick our the half reactions in Table 3.1 that involve the given oxidizing or reducing agents and list them, along with their E^(@) value increases (i.e. becomes more positive) whereas the strength of a reducing agent increases as the E^(@) value decreases (i.e. becomes more negative).

Justify the following raection as redox reaction. 2 Na(s) + S(s) rarr Na_2 S(s) Find out the oxidizing and reducing agents.