Answer to Question #159538 in Chemistry for Sydney

Question

Consider the decomposition reaction:           CuCO₃.Cu(OH)₂   →  2CuO + CO₂ + H₂O             

       Calculate the theoretical yield of carbon dioxide, CO₂, produced by the decomposition reaction if 10.0 g of CuCO₃.Cu(OH)₂ are consumed. Copper (II) carbonate – copper (II) hydroxide has a molar mass of 221.13 g/mol.

 

Answer 1

The balanced reaction equation is:

 CuCO₃.Cu(OH)₂   →  2CuO + CO₂ + H₂O  .

As one can see from the equation, 1 mole of Copper (II) carbonate – copper (II) hydroxide produces 1 mole of carbon dioxide. The number of the moles of CuCO₃.Cu(OH)₂ is its mass divided by its molar mass:

$n(CuCO_3\cdot Cu(OH)_2)= \frac{m}{M} = \frac{10}{221.13}=0.04522$ mol.

Therefore, the number of the moles of carbon dioxide equals 0.04522 mol also. Its mass will be the number of the moles times its molar mass 44.01 g/mol:

$m(CO_2) = n\cdot M = 0.04522\cdot44.01 = 1.99$ g.

Answer: if 10.0 g of CuCO₃.Cu(OH)₂ are consumed, the theoretical yield of carbon dioxide, CO₂, produced by the decomposition reaction is 1.99 g.