A sample of magnesium is partially oxidised to magnesia. 3 grams of such sample is treated with excess dilute sulphuric acid and the hydrogen collected measures 1.12 L at STP. What is the weight ratio of metal and metal oxide in the sample?

A sample of magnesium is partially oxidised to magnesia. 3 grams of su

1.	A sample of magnesium is partially oxidised to magnesia. 3 grams of such sample is treated with excess dilute sulphuric acid and the hydrogen collected measures 1.12 L at STP. What is the weight ratio of metal and metal oxide in the sample?
Answer» Solution :Reaction of sulphuric ACID with COMPONENTS is given as `MG+H_(2)SO_(4) to MgSO_(4)+H_(2)` `MgO+H_(2)SO_(4) to MgSO_(4)+H_(2)O` 1 mole of `H_(2)=` 1 mole of Mg 22.4 of `H_(2)` at STP=24 g of Mg 1.12 L of `H_(2)` at =STP=? Weight of magnesium in given sample= `(1.12)/(22.4) XX 24=1.2" grams"` Weight of MgO in given sample `=3-1.2=1.8` grams Weight ratio of Mg and MgO =1.2 : 1.8=2:3