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Question

A 0.60 g sample consisting of only CaC2O4 and MgC2O4 is heated at 500 oC converting the two salts to CaCO3 and MgCO3. The sample then weight 0.465 g. If the sample had been heated to 900 oC, where the products are CaO and MgO, what would the mixtures of oxide have weighed (in grams)?
Report your answer upto two decimal only.


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Solution

Let x g is the weight of CaC2O4 and (0.6x) g is the weight of MgC2O4
CaC2O4Δ−−−CaCO3+CO

MgC2O4Δ−−−MgCO3+CO
Weight of CaCO3 produced=x128×100

Weight of MgCO3 produced =(0.6x)112×84
x128×100+(0.6x)112×84=0.465
x=0.48 g
Due to further heating,
CaCO3Δ−−−−CaO+CO2x128
MgCO3Δ−−−−−MgO+CO2(0.6x112)
Weight of CaO and MgO produced,
=0.48128×56+0.12112×40=0.252 g


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