Question

How many moles of oxygen are produced when 5.12 moles of magnesium chlorate decomposes into magnesium chloride and oxygen?

Answer 1

The  moles   of  oxygen  produced  is  calculated  as    follows

write  a  balanced  reacting  equation,  that  is

Mg(ClO3)2  ---->MgCl2  +  3O2

from  the  equation  above  the  reacting  ratio  of  Mg(ClO3)2  to  O2  is  1:   3  therefore  the  moles  of  O2  produced  =  5.12  moles  x3  =15.36  moles

Answer 2

The moles of oxygen produced has been 15.36 mol.

The decomposition of Magnesium chlorate has been given as:

$\rm Mg(ClO_3)_2\;\rightarrow\;MgCl_2\;+\;3\;O_2$

From the balanced chemical equation, decomposition of 1 mole of magnesium chlorate results in the formation of 3 moles of oxygen.

Computation for moles of Oxygen produced

The available moles of magnesium chlorate has been 5.12 mol.

The moles of oxygen produced has been given as:

$\rm 1\;mol\;Mg(ClO_3)_2=3\;mol\;O_3\\ 5.12\;mol\;Mg(ClO_3)_2=5.12\;\times\;3\;mol\;O_2\\ 5.12\;mol\;Mg(ClO_3)_2=15.36\;mol\;O_2$

The moles of oxygen produced has been 15.36 mol.

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