Determine the mass of hydrogen for the reaction with copper oxide weighing 21.7 grams.

Divalent copper oxide is reduced with hydrogen gas when heated. This synthesizes metallic copper and water. The reaction is described by the following chemical reaction equation:

CuO + H2 = Cu + H2O;

Cupric oxide reacts with hydrogen in equal (equivalent) molar amounts. In the course of the reaction, the same equal chemical amounts of copper and water are synthesized.

Let’s calculate the chemical (molar) amount of copper oxide.

For this purpose, we divide the weight of the oxide by the weight of 1 mole of oxide.

M CuO = 64 + 16 = 80 grams / mol;

N CuO = 21.7 / 80 = 0.27125 mol;

Thus, it is possible to carry out the reduction of 0.27152 mol of copper oxide and obtain 0.27125 mol of copper.

The same amount of hydrogen gas will be required. Let’s find its weight.

N H2 = 0.27125 mol;

M H2 = 2 grams / mol;

V H2 = 0.27125 x 2 = 0.5425 grams;

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