Answers:
<em><u>a. Moles of oxygen formed:</u></em><u> 0.670 mol</u>
<em><u>b. Moles of water formed:</u></em><u> 1.34 mol</u>
<em><u>c. Mass of water formed:</u></em><u> 24.1 g</u>
<em><u>d. Mass of oxygen formed:</u></em><u> 21.4 g</u>
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Explanation:
Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.
The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:
The mole ratios derived from that balanced chemical equation are:
- 2 mol H₂O₂ : 2 mol H₂O : 1 mol O₂
<em><u>a. Moles of oxygen formed</u></em>
- Set the proportion using the theoretical mole ratio of H₂O₂ to O₂ and the amount of moles of dyhydrogen dioxide that react:
When you solve for x, you get:
- x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂
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<em><u>b. Moles of water formed</u></em>
- Set the proportion using the theoretical mole ratio of H₂O₂ to H₂O and the amount of moles of dyhydrogen dioxide that react:
When you solve for x, you get:
- x = 1.34 mol H₂O₂ × 2 mol H₂O / 2 mol H₂O₂ = 1.34 mol H₂O
<em><u>c. Mass of water formed</u></em>
Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:
- Molar mass of water = 18.015 g/mol
- Number of moles = mass in grams / molar mass
⇒ mass in grams = number of moles × molar mass
⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g
<em><u>d. Mass of oxygen formed</u></em>
Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.
- Molar mass of O₂ = 32.00 g/mol
- mass = molar mass × number of moles
- mass = 32.00 g/mol × 0.670 mol = 21.4 g.