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Question

# A 0.60g sample consisting of only CaC2O4 and MgC2O4 is heated at 500∘C, converting the two salts of CaCO3 and MgCO3. The sample then, weighs 0.465g. If the sample had been heated to 900∘C, where the products are CaO and MgO, what would the mixtures of oxides have weighed?

A
0.12g
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B
0.21g
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C
0.252g
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D
0.3g
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Solution

## The correct option is C 0.252gLet xg is the weight of CaC2O4 and (0.6−x) g be the weight of MgC2O4.The reactions are as follows:CaC2O4△−→CaCO3+CO2MgC2O4△−→MgCO3+CO2Weight of CaCO3 produced=x128×100.Weight of MgCO3 produced=(0.6−x)112×84.∴x128×100+(0.6−x)112×84=0.465.Therefore, x=0.48gDue to further heating,CaCO3△−→CaO+CO2 - x128MgCO3△−→MgO+CO2 - 0.6−x112Weight of CaO and MgO produced =0.48128×56+0.12112×40=0.252g.Hence, option C is correct.

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