Question

a 15.7 g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hcl. the resulting reaction produces 5.03 l of carbon dioxide gas at 28 °c and 657 torr. write a balanced chemical equation for the reaction that takes place between magnesium carbonate and hcl. include physical states. chemical reaction: write a balanced chemical equation for the reaction that takes place between calcium carbonate and hcl. include physical states. chemical reaction: calculate the total number of moles of carbon dioxide that forms from these reactions. moles of carbon dioxide: mol assuming the reactions are complete, calculate the precentage by mass of magnesium carbonate and calcium carbonate in the mixture. magnesium carbonate: % calcium carbonate: %

Answer 1

Calcium carbonate breaks down into 2HCl + MgCO3 ==> MgCl2 + CO2 + H2O when it is heated.

Balanced equation: 2HCl + CaCO3 ==> CaCl2 + CO2 + H2O

I'll have to make a guess as to what the units are since you nearly entirely left them out.

Is that 1.74 mols, 1.74 g, or 1.74 litres of carbon dioxide? Is that 741 mm Hg and 29 °C?

PV = nRT

n = PV/RT

n = (1 atm x 741 mm x 760 mm)(1.74 L)/(0.0821 L atm/Kmol) (302K)

n = 0.0684 moles of CO2

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