Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 20.0 g of dinitrogen monoxide decomposes?
To find the number of grams of oxygen gas formed when 20.0 g of dinitrogen monoxide decomposes, we first need to find the molar masses of the substances involved:
N2O (dinitrogen monoxide) = 44.02 g/mol
N2 (nitrogen gas) = 28.02 g/mol
O2 (oxygen gas) = 32.00 g/mol
Now we can set up a ratio using the balanced chemical equation for the decomposition of dinitrogen monoxide:
2N2O -> 2N2 + O2
From the balanced equation, we see that 1 mole of dinitrogen monoxide decomposes to form 1 mole of oxygen gas. Therefore, the molar ratio of N2O to O2 is 1:1.
Now we can calculate the number of moles of oxygen gas formed from the given mass of dinitrogen monoxide:
20.0 g N2O * (1 mol N2O / 44.02 g N2O) * (1 mol O2 / 1 mol N2O) = 0.454 mol O2
Finally, we can find the mass of oxygen gas formed:
0.454 mol O2 * 32.00 g/mol = 14.5 g O2
Therefore, when 20.0 g of dinitrogen monoxide decomposes, 14.5 grams of oxygen gas are formed.