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mr Goodwill [35]
3 years ago
15

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

rogen monoxide decomposes?
Chemistry
1 answer:
lina2011 [118]3 years ago
5 0

Answer:

There is formed 3.6352 grams of oxygen

Explanation:

<u>Step 1</u>: The balanced equation

2N2O(g)⇔2N2(g)+O2(g)

<u>Step 2</u>: 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

<u>Step 3</u>: 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

<u>Step 4:</u> 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

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Explanation:

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At 311 K, this reaction has a K c value of 0.0111 . X ( g ) + 2 Y ( g ) − ⇀ ↽ − 2 Z ( g ) Calculate K p at 311 K. Note that the
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Answer:

K_{p}=4.35\times 10^{-4}

Explanation:

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