Question

A 2.077 g sample of an element, which has an atomic mass between 40 and 55, reacts with oxygen to form 3.708 g of an oxide. Determine the formula mass of the oxide (and identify the element).

Answer 1

Vanadium  and the oxide is V2O5.

What is the oxide?

We have the information that the  element which has an atomic mass between  40 and 55  reacts with oxygen. This compound must e ionic so we can write; 2M + x/2O2 --->M2Ox

Mass of oxygen utilized in the reaction is; 3.708 g - 2.077 g  = 1.631 g

Number of moles of oxygen used = 1.631 g/32g/mol = 0.051 moles

Number of moles of the metal =   2.077 g/M

Thus;

2.077 g/M  * x/4 = 0.051 moles

2.077x/4M =  0.051 moles

2.077x = 0.204M

M = 2.077x /0.204

M = 10.181x

Given that x could be 4 or 5, we have to agree that x =5 which gives a mass of  50.93 thus M is Vanadium  and the oxide is V2O5.

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