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kondaur [170]
3 years ago
11

What happens when mercury oxide is heated?

Chemistry
1 answer:
weeeeeb [17]3 years ago
7 0
It produces mercury and oxygen gas.
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Gas, Solid, or liquid

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Dihydrogen dioxide decomposes into water and oxygen gas. Calculate the amounts requested if 1.34 moles of dihydrogen dioxide rea
a_sh-v [17]

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>

<u></u>

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:

2H_2O_2(l)\rightarrow 2H_2O(l)+O_2(g)

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:

2\text{ mol }H_2O_2/1\text{ mol }O_2=1.34\text{ mol }H_2O_2/x

When you solve for x, you get:

  • x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂

<u />

<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:

2\text{ mol }H_2O_2/2\text{ mol }H_2O=1.34\text{ mol }H_2O_2/x

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.
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Using cross multiplication:

1.0 mole of Fe(NO₃)₃ contains → 6.022 x 10²³ formula units.

??? mole of Fe(NO₃)₃ contains → 9.69 x 10²⁵ formula units.

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The second option

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