Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the decomposition of dinitrogen monoxide is:

N2O(g) → N2(g) + O2(g)

From the equation, we can see that the ratio of oxygen to dinitrogen monoxide is 1:2.

To find the mass of oxygen produced, we need to first calculate the number of moles of dinitrogen monoxide:

mol N2O = mass/molar mass = 10.0 g / 44.01 g/mol = 0.227 mol N2O

Using the mole ratio from the balanced equation, we can then calculate the number of moles of oxygen produced:

mol O2 = 0.5 mol N2O = 0.5 x 0.227 mol = 0.114 mol O2

Finally, we can convert the number of moles of oxygen to grams using the molar mass of oxygen:

mass O2 = mol O2 x molar mass O2 = 0.114 mol x 32.00 g/mol = 3.64 g

Therefore, the answer is B.

Dinitrogen Monoxide Gas Decomposes to Form Nitrogen Gas and Oxygen