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2.5 g of a mixture of BaO and CaO when treated with an  excess of H2SO4,...

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user2970017 | eNotes Newbie

Posted June 28, 2013 at 7:57 AM via web

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2.5 g of a mixture of BaO and CaO when treated with an 
excess of H2SO4, produced 4.713 g ofthe mixed sulphates.
Find the percentage of BaO present in the mixture

Tagged with science, stoichiometry

1 Answer | Add Yours

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jeew-m | College Teacher | (Level 1) Educator Emeritus

Posted June 28, 2013 at 8:35 AM (Answer #1)

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`BaO+H_2SO_4 rarr BaSO_4+H_2O`

`CaO+H_2SO_4 rarr CaSO_4+H_2O`

 

Molar mass in g/(mol)

`BaO = 153`

`CaO = 56`

`CaSO_4 = 136`

`BaSO_4 = 233`

 

Mole ratio

`BaO:BaSO_4 = 1:1`

`CaO:CaSO_4 = 1:1`

 

Let us say we have xg of BaO in the mixture. So we should have (2.5-x)g of CaO.

Amount of BaO moles` = x/153`

Amount of CaO moles` = (2.5-x)/56`

 

Since mole ratio is `1:1` ;

Amount of `BaSO_4 ` moles `= x/153`

Amount of `CaSO_4` moles `= (2.5-x)/56`

 

Weight of `BaSO_4 = x/153xx233`

Weight of `CasO_4 = (2.5-x)/56xx136`

 

But the weight of the sulphate mixture is 4.713g

`x/153xx233+(2.5-x)/56xx136 = 4.713`

`x = 1.5`

 

So the weight of BaO is 1.5g.

Percentage weight of BaO `= 1.5/2.5xx100% = 60%`

 

So we have 60% of BaO in the mixture.

 

Assumption

The mixture only contains BaO and CaO without any impurities.

 

 

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