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

`m_(O_2)=87.2gO_2`

Step-by-step 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*(1molH_2O)/(18.02gH_2O)*(1molO_2)/(2molH_2O)*(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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