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Question

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

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

## The correct option is C 0.252 gLet x g is wt. of CaC2O4 and (0.6−x) g wt. of MgC2O4 CaC2O4△−→CaCO3+CO2 MgC2O4△−→MgCO3+CO2 wt. of CaCO3 produced =x128×100 wt. of MgCO3 produced =(0.6−x)112×84 ∴x128×100+(0.6−x)112×84=0.465 x=0.48 g Due to further heating, CaCO3△−→CaO+CO2 x128 MgCO3△−→MgO+ CO2 (0.6−x112) Putting the value of x and finding wt. of CaO and MgO produced =0.48128×56+0.12112×40=0.252 g

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