If $$10$$ g of Ag reacts with $$1$$ g of sulphur, the amount of $$Ag2S$$ formed will be [Atomic weight of Ag $$=$$ $$108$$, S $$=$$ $$32$$] ?

Question

If $$10$$ g of Ag reacts with $$1$$ g of sulphur, the amount of $$Ag2S$$ formed will be [Atomic weight of Ag $$=$$ $$108$$, S $$=$$ $$32$$] ?

Infinity Learn · Accepted Answer

Explanation :  $$2$$  Ag $$+$$  S  →  $$Ag2S2$$  ×  $$108$$  g  of Ag reacts with $$32$$  g of $$sulphur10$$ g  of Ag  reacts  with $$32216$$ ×  $$10=320216$$ > $$1$$ gIt means ‘S’ is limiting $$reagent32$$ g of S reacts to form $$216$$ $$+$$ $$32$$ $$=$$ $$248$$ g of $$Ag2S1$$ g of S reacts to form $$24832=7.75$$  gAlternative method :  neq of Ag $$=$$ $$10108=0.0925$$;neq of S $$=$$ $$116=0.0625$$ neq  $$=$$ number  of  equivalentsSince  neq of S is  less than neq of Ag⇒  $$0.0625$$ eq of Ag will  react  with  $$0.0625$$  eq  of  S to  $$form0.0625$$  eq  of $$Ag2SHence$$,  amount of $$Ag2S$$  $$=$$  neq ×  Eq.  wt.  of  $$Ag2S=0.0626$$  ×  $$124=7.75g$$

If 10 g of Ag reacts with 1 g of sulphur, the amount of Ag2S formed will be [Atomic weight of Ag = 108, S = 32] ?

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