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meriva
3 years ago
7

Which statement below BEST describes the difference between mixtures and pure substances? Group of answer choices Mixtures are m

ade of a single kind of matter but a pure substance is two or more substances that are chemically bonded. Pure substances can be physically separated but mixtures cannot be physically separated. Pure substances are not created through a chemical reaction and mixtures are the result of a chemical reaction. Mixtures can be physically separated but pure substances cannot be physically separated.
Chemistry
1 answer:
lianna [129]3 years ago
6 0

Answer:  <u>Mixtures can be physically separated but pure substances cannot be physically separated.</u>

Explanation: Mixtures can be physically separated by using methods that use differences in physical properties to separate the components of the mixture, such as evaporation, distillation, filtration and chromatography. A pure substance, any compound or element, can't be separated into different atoms by physical methods. Pure substances are compounds and elements (made up of the same atom or same molecule respectively), while mixtures are an assortment of different substances put together. Hope this helps ^-^.

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posledela
The answer is the second option. The given conversion from L to dm3 is actually confusing. Just remember that 1 L = 1000 cm3.
Simply, multiply 2.6 by 1000 and we get 2600 cm. Converting this to scientific notation, we get the answer:
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6 0
3 years ago
By process of incineration, a mystery substance is empirically determined to contain 40.00% carbon by weight, 6.67% hydrogen, an
Keith_Richards [23]

Answer:

C₂H₄O₂

Explanation:

Step 1: Divide each percentage by the atomic mass of the element

C: 40.00/12.01 = 3.331

H: 6.67/1.01 = 6.60

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Step 2: Divide all the numbers by the smallest one

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H: 6.60/3.331 ≈ 2

O: 3.333/3.331 ≈ 1

The empirical formula is CH₂O, with a molecular weight of 12 g/mol + 2 × 1 g/mol + 16 g/mol = 30 g/mol. The molecular weight of the compound must be a product of 30, such as 60 (between 55 and 62 g/mol). Since we have to multiply by 2 (30 to 60) to get to the molecular weight of the compound, we also have to multiply the empirical formula by 2 to get the chemical formula of the compound.

CH₂O × 2 = C₂H₄O₂

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hope this helped

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ok you answer is probably A

if wrong C maybe

~hope~

6 0
3 years ago
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