A 2.18 g sample contains a mixture of XO and X2O3. It reacts with 0.01 – InterviewSolution

1.	A 2.18 g sample contains a mixture of XO and X2O3. It reacts with 0.015 moles of K2Cr2O7 to oxidize the sample completely to form XO−4 and Cr3+. If 0.0187 moles of XO−4 are formed, what is the atomic mass of X?
Answer» A $2.18 g$ sample contains a mixture of $X O$ and $X_{2} O_{3} .$ It reacts with 0.015 moles of $K_{2} C r_{2} O_{7}$ to oxidize the sample completely to form $X O_{4}^{-}$ and $C r^{3 +}$ . If 0.0187 moles of $X O_{4}^{-}$ are formed, what is the atomic mass of X?

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