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vlada-n [284]
3 years ago
5

A 5.687 g sample of iron reacts with oxygen, forming an iron oxide. The final mass of the iron oxide is 8.131 g. What is the for

mula of the iron oxide
Chemistry
1 answer:
Klio2033 [76]3 years ago
6 0

Answer:

Fe₂O₃

Explanation:

Mass of Iron = 5.687 g

Mass of Iron oxide = 8.131 g

Mass of Oxide = Mass of Iron oxide - Mass of Iron

Mass of oxide = 8.131 - 5.687 = 2.444 g

Moles of Iron =  Mass / Molar mass = 5.687 / 55.845 = 0.1018 moles

Moles of Oxide  =  Mass / Molar mass = 2.444 / 16 = 0.15275 moles

To determine the formular, we have to find the smallest whole number ration that exists between the elements.

To do that, we divide by the smallest number;

Iron = 0.1018 / 0.15275 = 0.6664 = 2/3 (Approximately)

Oxygen = 0.15275 / 0.15275 = 1

To get the smallest whole number ratio, multiply all through by 3.

Iron = 2/3 * 3 = 2

Oxygen = 1 * 3 = 3

The formular will be;

Fe₂O₃

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Why is chlorine called non-metal?​
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8 0
3 years ago
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What is the pH of a solution of 0.800 M KH2PO4, potassium dihydrogen phosphate?
Nookie1986 [14]
KH₂PO₄ hydrolyzes as;
H₂PO₄⁻ + H₂O ↔ H₃PO₄ + OH⁻
Let x amount of H₂PO₄⁻ has reacted with water then,
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[H₂PO₄⁻] = 0.8-x M
Kb₁ = x² / (0.8 - x)
Given Ka₁ = 7.5 x 10⁻³
so Kb₁ = 1 x 10⁻¹⁴ / (7.5 x 10⁻³) = 1.33 x 10⁻¹²
From this information:
1.33 x 10⁻¹² = x² / 0.8
x = [OH⁻] = 1.03 x 10⁻⁶ M
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If nitrogen and hydrogen combine in a combustion reaction, what would the product of the reaction be?
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CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l)

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