What is the mass of copper if 16 g of copper oxide is reduced with hydrogen?

What is the mass of copper if 16 g of copper oxide is reduced with hydrogen? How much hydrogen will be required for recovery?

Given:

m (CuO) = 16 g

Find:

m (Cu) -?

V (H2) -?

Solution:

1) We compose the reaction equation corresponding to the condition of the problem:

CuO + H2 = H2O + Cu;

2) Find the amount of copper oxide contained in 16 grams of the substance:

n (CuO) = m: M = 16 g: 80 g / mol = 0.2 mol;

3) Find the mass of copper released during the reaction according to the first logical equality:

if 1 mol of CuO gives 1 mol of Cu,

then 0.2 mol CuO will give x mol Cu,

then x = 0.2 mol.

m (Cu) = n * M = 0.2 mol * 64 g / mol = 12.8 g;

4) Find the volume of consumed hydrogen according to the second logical expression:

if 1 mol of CuO requires 1 mol of H2,

then 0.2 mol CuO will require x mol H2,

then x = 0.2 mol.

V (H2) = n * Vm = 0.2 mol * 22.4 L / mol = 4.48 L;

Answer: m (Cu) = 12.8 g; V (H2) = 4.48 liters.