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Arsenic sulphide (As_(2)S_(3)) reacts with sulphuric acid (H_(2)SO_(4)) to form H_(3)AsO_(4) (Arsenic acid) and sulphur - dioxide (SO_(2)). What will be the coefficient of H_(2)SO_(4),H_(3)AsO_(4)andSO_(2) respectively in the balanced reaction ? |
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Answer» 11, 2 and 14 (x) Oxidation Part : (i) `As_(2)S_(3)toH_(3)AsO_(4)+SO_(2)` (ii) `As_(2)S_(3)to2II_(3)AsO_(4)+2SO_(2)` (Balance As, S) (iii) `underset(2(+3))underset(DARR)(As_(2))underset(+(-2)3)underset(darr)(S_(3))to2H_(3)Asunderset(2(+5))underset(darr)(O_(4))+underset((+4)3)underset(darr)(3SO_(2))` = + 6 - 6= 10 + 12 = Zero `to` = 22 `therefore` Oxidation number is up by (22) (y) Reduction Part : `underset((+6))underset(darr)(H_(2)SO_(4))tounderset((+4))underset(uarr)(SO_(2))` ... (Reduction) Oxidation no. is down by (2) in Reduction part (z) Balance of change of oxidation number oxidation part `xx` 1 and reduction part `xx` 11 `As_(2)S_(3)to2H_(3)AsO_(4)+2SO_(2)""...(i)` `11H_(2)SO_(4)to11SO_(2)` ... (Reduction) ...(ii) `z(i)+z(ii)" "As_(2)S_(3)+11H_(2)SO_(4)to2H_(3)AsO_(4)+14SO_(2)` Balancing H and O by adding `8H_(2)O` we get BALANCED redox EQUATION... `As_(2)S_(3)+11H_(2)SO_(4)to2H_(3)AsO_(4)+14SO_(2)+8H_(2)O` `therefore` Coefficient of `H_(2)SO_(4)` = 11 `therefore` Coefficient of `H_(3)AsO_(4)=2` `therefore` Coefficient of `SO_(2)` = 14 |
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