It takes 0.15 mol of ClO− to oxidise 12.6 g of chromium oxide of a s – InterviewSolution

1.	It takes 0.15 mol of ClO− to oxidise 12.6 g of chromium oxide of a specific formula to Cr2O2−7. ClO− became Cl−. The formula of the oxide is:(Atomic weight: Cr=52,O=16)
Answer» It takes $0.15 m o l$ of $C l O^{-}$ to oxidise $12.6 g$ of chromium oxide of a specific formula to $C r_{2} O_{7}^{2 -}$ . $C l O^{-}$ became $C l^{-}$ . The formula of the oxide is: (Atomic weight: $C r = 52, O = 16$ )

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