Question

Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is 2H2O(g)⟶2H2(g)+O2(g) Calculate how many grams of O2(g) can be produced from 98.2 g H2O(g).

Answer 1

Answer:

$m_{O_2}=87.2gO_2$

Explanation:

Hello.

In this case, given the chemical reaction, we can compute the grams of oxygen by using the 98.2 g of water via the 2:1 mole ratio between them, the molar mass of water that is 18.02 g/mol, the molar mass of gaseous oxygen that is 32.00 g/mol and the following stoichiometric procedure relating the given information:

$m_{O_2}=98.2gH_2O*\frac{1molH_2O}{18.02gH_2O}*\frac{1molO_2}{2molH_2O}*\frac{32.00gO_2}{1molO_2} \\\\m_{O_2}=87.2gO_2$

In which the result is displayed with three significant figures because the given mass of water 98.2 g, has three significant figures too.

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