You carefully weigh out 13.00 g of CaCO3 powder and add it to 52.65 g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 60.32

g. The relevant equation isCaCO3 (s) + 2HCl (aq) ? H2O (l) + CO2 (

g.+CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units.

Question

Ezequiel Mcdowell

Chemistry

7 December, 05:40

You carefully weigh out 13.00 g of CaCO3 powder and add it to 52.65 g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 60.32

g. The relevant equation isCaCO3 (s) + 2HCl (aq) ? H2O (l) + CO2 (

g.+CaCl2 (aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction? Express your answer to three significant figures and include the appropriate units.

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Answers (1)

Know the Answer?

Myla Harrington · Answer 1

CaCO₃ + 2HCl = CaCl₂ + CO₂ + H₂O

n (CaCO₃) = m (CaCO₃) / M (CaCO₃)

n (CaCO₃) = 13.00/100.09=0.1299 mol

Δm=13.00+52.65-60.32=5.33 g

m (CO₂) = 5.33 g

n (CO₂) = 5.33/44.01=0,1211 mol

w=0.1211/0.1299=0,9323 (93.23%)