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spin [16.1K]
3 years ago
10

Examples of pure and impure substances

Chemistry
2 answers:
erastova [34]3 years ago
8 0
Pure- table salt
Impure- vegetable oil
Sladkaya [172]3 years ago
8 0

Examples of pure substances are water, diamond, table salt

Examples of impure substances are muddy water, air, sugar in water

<u>Explanation</u>:

  • A pure substance is one that is made up of only one element or one chemical compound. It has no impurities. They can be elements or compounds.
  • It has definite properties and composition.
  • Examples are water, diamond, table salt, etc.
  • An impure substance is one that is made up of two or more elements or compounds that are not chemically bonded. It is a mixture.
  • It has no definite composition or properties.
  • Examples are muddy water, sugar in water, air, etc.
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What amount of energy is required to completely ionize 27.8 grams of carbon atoms in the gas phase (c(g)) if the ionization ener
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In the lab you measure a clean dry crucible and cover to be 24.36 grams. You obtain a 2cm piece of pure magnesium metal. After s
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Answer:

1) 0.3g Mg

2)0.5g MgO

3)0.2g O

4)0.01mol Mg & 0.01mol O

5)0.01mol MgO

6) Empirical formula MgO

Explanation:

The mass og Mg is obtained by substracting 24.36g from 24.66g:

24.66 - 24.36 = 0.3g Mg

The ignition of Mg means that it's reacting with oxygen to form an oxide. The increase in the crucible mass after the Mg ignition is due to the addition of oxygen. However, the addition of few drops of water produces a new compound: a hydroxide. According to the oxidation state og Mg (2+), the only magnesium oxide possible is MgO. It happens because the oxidation state of oxygen in oxides is 2-. Which means that just one oxygen atom is required to electrically neutralize one magnesium atom.

We can use a conversion factor to know how much MgO is made from from 0.3 g of Mg:

0.3g Mg*\frac{16gO}{24.3gMg}= 0.2g O

Thereby the mass of the oxide is 0.2g O + 0.3g Mg = 0.5g MgO

We convert the mass of oxygen and magnesium to the respective amounts in moles by using conversion factors:

0.2g O*\frac{1 mol O}{16g O}= 0.01mol O

0.3g Mg*\frac{1mol Mg}{24.3g Mg}= 0.01mol Mg

The moles of MgO can be obtained from:

0.5g MgO*\frac{1mol MgO}{40.3g MgO}= 0.01mol MgO

To obtain the empirical formula, the amount fo moles of each elements must be divided by the smallest one, in this case, 0.01.

The result for both number of  Mg atoms and O atoms is 1. This can be interpreted to mean that there is a Mg atom for each O atom forming the  formula unit of the compound.

The step when water is added to the compound resulting after heating does not affect the calculations necessary for the magnesium oxide.

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Active mass = 0.75mol/1.5L

Active mass = 0.5mol/L

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