Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 5.00 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 molar ratio of O2 formed to N2O decomposed is 1:1. That means, for every 1 mole of N2O decomposed, 1 mole of O2 is formed.

To find the number of moles of N2O in 5.00 g, we need to divide the given mass by the molar mass of N2O:
Number of moles of N2O = 5.00 g / 44.013 g/mol = 0.1135 mol

Since the molar ratio of O2 to N2O is 1:1, the number of moles of O2 formed will be equal to the number of moles of N2O decomposed:
Number of moles of O2 = Number of moles of N2O = 0.1135 mol

Finally, we can use the molar mass of O2 to convert the number of moles to grams:
Mass of O2 = 0.1135 mol x 32.00 g/mol = 3.632 g
Rounding this answer to two significant figures gives us: 1.82 g

Dinitrogen Monoxide Gas Decomposes to Form Nitrogen Gas and Oxygen