Question

# A 1004.0g sample of calcium carbonate that is 95.0% pure gives 225L of CO_{2} at STP when reacted with an excess ofhydrochloric acid. What is the density (in g/L) of the carbondioxide?

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A 1004.0g sample of calcium carbonate that is 95.0% pure gives 225L of $$\displaystyle{C}{O}_{{{2}}}$$ at STP when reacted with an excess ofhydrochloric acid.
What is the density (in g/L) of the carbondioxide?

2021-04-09

Don't gases have a molar density of 1mol/ 22.4L at STP? Can't thatbe converted to grams per liter.
Here is the long way: $$\displaystyle{C}{a}{C}{O}_{{{3}}}+{2}{H}{C}{I}+{C}{a}{C}{I}{2}+{C}{O}_{{{2}}}+{H}{20}$$
Thus 1004 grams of calcium carbonate only 95% pure:
grams of $$CaCO_3: 0.95(1004.0g)$$
Can convert that to grams of carbon dioxide:
$$0.95(1004.0g CaCO_3) * (1mol CaCO_3/100g CaCO_3) * (1 mol CO_2/1molCaCO_3) * (44 g CO_2/ 1 mol CO_2) = 419.7$$ grams
That is 419.7 grams in 225 L, so density = 419.7g/225L = 1.87g/L