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

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

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