The volume of hydrogen required for the complete reduction of zinc oxide obtained during the decomposition

The volume of hydrogen required for the complete reduction of zinc oxide obtained during the decomposition of 0.2 mol of zinc hydroxide is equal to.

To solve the problem, we compose the equation of the process:

Y = 0.2 mol

Zn (OH) 2 = ZnO + H2O – decomposition, zinc oxide obtained;

Chl -?

ZnO + H2 = Zn + H2O – reduction, zinc was formed;

Let’s determine the amount of substances:
Y (ZnO) = 0.2 mol;

Y (H2) = 0.2 mol since the amount of substances is 1 mol.

We find the volume of the original substance:
V (H2) = 0.2 * 22.4 = 4.48 L

Answer: the volume of hydrogen is 4.48 liters.