If 3.00 mol of #CaCO_3# undergo decomposition from #CaO# and #CO_2# how many grams of #CO_2# are produced?

1 Answer
anor277
Mar 22, 2016

Clearly, #3.00# #mol# of carbon dioxide gas are evolved.

Explanation:

We need the stoichiometric equation;

#CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr#

You have to heat this fairly fiercely, but clearly, quantitative reaction indicates that 1 mol of carbon dioxide is evolved per mole of calcium carbonate.

#CaO# dissolves in water to give limewater, aqueous calcium hydroxide (this is sparingly soluble, so filter it);

#CaO(s) + H_2O(l) rarr Ca(OH)_2(aq)#

If filtered limewater is treated with carbon dioxide, calcium carbonate is reformed, and precipitates from solution as a milky white solid:

#Ca(OH)_2(s) + CO_2(g) rarr CaCO_3(s)darr + H_2O(l)#

All of these equations should be informed by doing the actual reactions in the laboratory. The best source of #CO_2# is sparkling water, the type you would drink for lunch; this is supersaturated with respect to carbon dioxide.

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