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Basile [38]
3 years ago
7

A __________ has distinct properties and composition that never vary. A) solution B) molecule C) pure substance D) heterogeneous

mixture
Physics
2 answers:
Nataly [62]3 years ago
8 0
Matter is defined as anything that has mass and occupies space, it may be classified into three states, solid, liquids or gases. Molecules is the smallest particle of an element that has the chemical properties of the element or the compound. it contains two or more atoms that are joined together. A pure substance is a matter that has distinct properties and a composition that does not vary from sample to sample. Thus the correct answer is C
sweet-ann [11.9K]3 years ago
6 0

Answer:

C) pure substance

Explanation:

Pure substance is any substance formed by only one type of molecule, of invariable and homogeneous chemical composition, which has constant physical and chemical properties. Pure substance may exist in more than one phase, but in such cases the phase composition will be the same.

In short, pure substance is all material with the following characteristics:

  • Structural units (molecules, ionic assemblies) chemically equal to each other.
  • Fixed composition, resulting in fixed properties such as density, melting and boiling point, etc. That is, these substance have distinct properties and composition that never vary.
  • The temperature remains unchanged from the beginning to the end of all your physical state changes (melting, boiling, solidifying, etc.).
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igor_vitrenko [27]

First, balance the reaction:

_ KClO₃   ==>   _ KCl + _ O₂

As is, there are 3 O's on the left and 2 O's on the right, so there needs to be a 2:3 ratio of KClO₃ to O₂. Then there are 2 K's and 2 Cl's among the reactants, so we have a 1:1 ratio of KClO₃ to KCl :

2 KClO₃   ==>   2 KCl + 3 O₂

Since we start with a known quantity of O₂, let's divide each coefficient by 3.

2/3 KClO₃   ==>   2/3 KCl + O₂

Next, look up the molar masses of each element involved:

• K: 39.0983 g/mol

• Cl: 35.453 g/mol

• O: 15.999 g/mol

Convert 10 g of O₂ to moles:

(10 g) / (31.998 g/mol) ≈ 0.31252 mol

The balanced reaction shows that we need 2/3 mol KClO₃ for every mole of O₂. So to produce 10 g of O₂, we need

(2/3 (mol KClO₃)/(mol O₂)) × (0.31252 mol O₂) ≈ 0.20835 mol KClO₃

KClO₃ has a total molar mass of about 122.549 g/mol. Then the reaction requires a mass of

(0.20835 mol) × (122.549 g/mol) ≈ 25.532 g

of KClO₃.

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