Heating 2.40 g of the oxide of metal x (molar mass of x = 55.9 g/mol) in carbon monoxide (co) yields the pure metal and carbon dioxide. the mass of the metal product is 1.68 g. from the data given, show that the simplest formula of the oxide is x2o3 and write a balanced equation for the reaction.

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

Explanation:

Let the molecular formula of the oxide of metal be

Mass of metal product = 1.68 g

Moles of metal X =

1 mol of metal oxide produces 2 moles of metal X.

Then 0.03005 moles of metal X will be produced by:

of metal oxide

Mass of 0.01502 mol of metal oxide = 2.40 g (given)

y = 2.999 ≈ 3

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.

answerambulatory;