Question

u. -4 3) Convert the following equations below to a net ionic equation and write it in the space provided. H2SO4 (aq.) + NaOH(aq.) → Na2SO4(aq.) + 2H2O(1) 4) Label the oxidation, reduction processes and oxidizing and reducing agents in the reaction given below a) Fe(s) + O2(g) → Fe2O3 (8)

Answer 1

And the given equation is- 9. " H2 504 (aq.) + Naokaq) Naz 504 (22.) +242 011) By balancing - H2SO4(69) + 2NaOH (24.) —— Maz S02(.) +214000 This peaction is an acid-base reaction. where H2SO4 behaves as acid and Naot - behaved as base to produce a salt il Na2SO4 and . solvent H2O. Now 12.50+ ioméses as 21+ + 5092 - Naoh ionises as % Nat & out Na2SO4 ionises as => 2 watt sop2- H2O remains as 620 . . so net ionic equation is- 24 traq) +504(09.) fzrácaq.) 17 #(29)47 2-3 . znacaq) + 50% (22.) +2+304) The given reaction is a pecs) + 02 (9) - FeO3(s) Odcidation Stoube of Fe changes from 'o' to +3. . So for Fecs) oxidation process. oxidation state of co-atom changes from o’to - 2 So for Oz (9) meduction process Here Oz(9) ordizes Fe(s) to re(11),50 02 is oxidising agent. and fels) reducees O to co, so Fecs) is reducing agent..