An unknown oxide of manganese is reacted with carbon to from manganese metal and `CO_(2)` Exactly `31.6g` of the oxide, `Mn_(x)O_(y)`, yielded `13.2g` of `CO_(2)`. The simplest formula of the oxide is `(Mn = 55)` :

What is the oxidation state of Manganese (Mn) in K_(2)MnO_(4) ?

On reduction with hydrogen , 3.6 g of an oxide of metal left 3.2 g of metal . If the simplest atomic weight of metal is 64, the simplest formula of the oxide is

On reduction with hydrogen , 3.6 g of an oxide of metal left 3.2 g of metal . If the simplest atomic weight of metal is 64, the simplest formula of the oxide is

On reduction with hydrogen, 3.6 g of an oxide of metal (M) left 3.2 g of the metal. If the atomic weight of the metal is 64. the formula of the oxide is

If 5.0 g of Al react with 4.45 g of O_(2) , empirical formula of aluminium oxide is

If 2.73g of oxide of vanadium contains 1.53g fo the metal vanadium, the empirical formula of the oxide is

On reduction with hydrogen, 3.6 g of an oxide of matel left 3.2 g of metal. If the vapour density of metal is 32 , the simplest formula of the oxide would be

An unknown sample weighing 1.5 g was found to contain only Mn and S. The sample was completely reacted with oxygen and it produced 1.22 g of Mn(II) oxide and 1.38 g of SO_(3) .What is the simplest formula for this compound? (MnS)