A mineral consists of an equimolar mixture of the carbonates of two bivalent metals. One metal is present to the extent of 12.5 by weight. 2.8g of the mineral on heating lost 1.32g of CO2. What is the % by weight of the other metal?
A
87.5
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B
35.71
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C
65.11
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D
23.21
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Solution
The correct option is D23.21 Let two equimolar carbonates are ACO3 and BCO3 Weight of metal A=2.8×12.5100=2.8×0.125=0.35g ACO3+BCO3→AO+BO+2CO2 Total two moles CO2−3 provide 2 moles of CO2 or 60 g CO2−3 provide 44 g of CO2 Total mass of CO2−3 required to be produced 1.32 g of CO2=6044×1.32=1.8 g weight of metal (A+B)=2.8−1.8=1g weight of B=1−0.35=0.65g % of B=0.652.80×100=23.21