What is the volume of carbon dioxide released at room temperature and pressure when 6.2 g of copper carbonate reacts with excess dilute sulfuric acid?

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Background Information

This is a neutralisation reaction between an acid (sulfuric acid) and a base (copper carbonate). When a carbonate reacts with an acid, the products are a salt, carbon dioxide and water.

carbonate + acid --> salt + carbon dioxide + water

ATTENTION:       If you are NOT familiarised with these reactions, I advise first to revise and then try to solve the question.


First thing to do when we tackle problem like this one is to write down the balanced equation (if it is not given)

CuCO3 + H2SO4 --> CuSO4 + CO2 + H2O

RFM (CuCO3) = 124 g mol-1

Number of moles of CuCO3 = 6.2 g / 124 g mol-1 = 0.05 mol

For every 1 mole of CuCO3, 1 mole of CO2 is produced (Using the stoichiometry of the equation)

Number of moles of CO2 = 0.05 mol

Volume of CO2 gas released = 0.05 mol * 24 dm3 = 1.2 dm3 = 12000 cm3

Andreas O. GCSE Chemistry tutor, GCSE Maths tutor, GCSE Physics tutor

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