Title Oxidising and Reducing Agent.pdf ✅

(a.) CO (b.) SO2 (c.) H S 2 (d.) PH3 [CG PET- 2011] (8.) Which of the following is reducing agent? (a.) LiAlH4 (b.) Zn HCl + (c.) Sn HCl + (d.) All of the above [CG PET -2007] (9.) Which of the following is the strongest oxidising agent? (a.) HOCl (b.) HClO2 (c.) HClO3 (d.) HClO4 [J & K CET-(2004)] (10.) In organic reactions, sodium in liquid ammonia is used as (a.) Reducing agent (b.) Hydrating agent (c.) Oxidizing agent (d.) Precipitating agent AP EAMCET- 2001 (11.) In which of the following reactions ozone acts as a reducing agent? (a.) BaO O BaO 2O 2 3 2 + → + (b.) 3 2 2 2 2HCl O Cl H O O + → + + (c.) PbS 4O PbSO 4O + → + 3 4 2 (d.) 3 2 2 2 2KI O H O 2KOH I O + + → + + AP EAMCET- 1999] (12.) In the following two reactions: (1) 2 2 2 2 2H O 2H O O → + (2) H O 2I 2H I 2H O 2 2 2 2 − + + + → + H O2 2 acts as (a.) An oxidizing agent (b.) A reducing agent (c.) Both oxidizing agent and reducing agent respectively (d.) Both reducing agent and oxidizing agent respectively [AP EAMCET- 1995]
ANSWER (1.) a (2.) b (3.) c (4.) a (5.) d (6.) c (7.) b (8.) d (9.) d (10.) a (11.) a (12.) a
EXPLANATION (1.) Hydrogen peroxide (H O2 2 ) both as oxidizing and reducing agent. H O2 2 oxygen has - 1 oxidation state lies between -2 to +2 . Therefore oxygen can be oxidized to O2 zero oxidation state acting as reducing agent or can be reduced to H O2 or OH− is -2 oxidation state acting as an oxidizing agent. (2.) The oxidation no. of P in H PO 3 4 , 3 1 4 2 0 ( ) ( ) 3 8 0 5 x x x + + + − = + − = = + P has its highest oxidation state +5 means cannot be further released electrons to act as a reducing agent therefore, act as an oxidizing. (3.) In the given reaction, Fe s CuSO aq FeSO aq Cu s ( ) + → + 4 4 ( ) ( ) ( ) Iron (Fe) displace copper (Cu) from its solution. Therefore, Copper is less reactive than iron. (4.) Li+ is the weakest oxidizing agent as it has most negative standard reduction potential. Lithium is small in size and high ionization enthalpy. Therefore lithium has a high tendency to lose electron in solution other an alkali metals. Hence, lithium is the weakest oxidizing agent. (5.) In reaction ZnO C Zn CO + → + , 'C' as a reduct (6.) In CO2 , the oxidation number of C , i.e., +4 is already the maximum and it cannot increase its oxidation number. Hence, does not act as a reducing agent. (7.) The oxidation no. ofsulphur lies from -2 to +6 . In SO2 the oxidation state of sulphur is +4 . Thus oxidation no. may increase or decrease. So it can behave as both oxidising agent as well as reducing agent. (8.) A substance which loses electrons to other substance in a redox reaction and gets oxidized to the higher valency state is called reducing agent. (a) LiAlH4 is reducing agent H − easily thought. (b) Zn HCl + is reducing agent reduce HCl . (c) Sn HCl + is reducing agent reduce HCl . (9.) Perchloric acid (HClO4 ) is the strongest acid among these acidic because the acidic character of oxoacid increases with increasing the oxidation no. of a particular halogen atom. (10.) In organic reaction sodium in liquid ammonia is used as reducing agent. Sodium is a strong electropositive element. (11.) 4 2 BaO O BaO 2O 2 3 2 + + + + ⎯⎯→