What mass of zinc must be dissolved in hydrochloric acid so that 14.4 g of copper oxide can be reduced with the obtained hydrogen (2)
The reduction reaction of copper oxide is described by the following chemical reaction equation.
CuO + H2 = Cu + H2O;
1 mole of metal oxide reacts with 1 mole of hydrogen. In this case, 1 mol of metal and 1 mol of water are synthesized.
Let’s calculate the chemical amount of a substance in 14.4 grams of metal oxide.
M CuO = 64 + 16 = 80 grams / mol;
N CuO = 14.4 / 80 = 0.18 mol;
The same chemical amount of hydrogen will be required.
The reaction between zinc and hydrogen chloride is described by the following chemical reaction equation.
Zn + 2HCl = ZnCl2 + H2;
1 mole of metal reacts with 2 moles of acid. In this case, 1 mol of salt is synthesized and 1 mol of gaseous hydrogen is released.
To obtain 0.18 mol of hydrogen, it is necessary to dissolve 0.18 mol of zinc.
Let’s calculate the mass of the metal.
M Zn = 65 grams / mol;
m Zn = 65 x 0.18 = 11.7 grams;
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