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?

There is formed 3.6352 grams of oxygen

Explanation:

Step 1: The balanced equation

2N2O(g)⇔2N2(g)+O2(g)

Step 2: Calculate moles of dinitrogen monoxide

Moles = mass/ Molar mass

Moles of N2O = 10 grams of N2O / 44.01 g/mole

Moles of N2O = 0.227 moles

Step 3: Calculate moles of oxygen

When 2 moles of N2O is consumed, there is produced 1 mole of O2 ( and 2 moles of N2)

That means for 0.2272 moles of N2O consumed, there is produced 0.1136 moles of O2

Step 4: Calculate mass of O2

mass of O2 = moles of O2 * Molar mass of O2

mass of O2 = 0.1136 moles * 32 g/moles

mass of O2 = 3.6352 grams

There is formed 3.6352 grams of oxygen

it's 3.2 on edge, i just took the test.