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3 years ago

A mixture in which particles are not evenly distributed and particles keep their unique properties.

Chemistry

2 answers:

zheka24 [161]3 years ago

6 0

im pretty sure that it is B

lina2011 [118]3 years ago

4 0

<h2>Answer : Option D) Heterogeneous mixture</h2><h3>Explanation : </h3>

A mixture in which particles are not evenly distributed and particles keep their unique properties are called as heterogeneous mixture.

Usually, in heterogeneous mixture the substances are not evenly distributed and they can be easily separated through any physical methods. Also the components retains their original/unique properties in the mixture. It usually contains various particles from different substances that are not uniformly distributed throughout the mixture.

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Which of the following would remain a liquid longer as temperature continues to drop?

viktelen [127]

I just took a test with this question and got the answer wrong for saying ethane. The correct answer is propane.

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3 years ago

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When 125 grams of FeO react with 25.0 grams of Al, how many grams of Fe can be produced? FeO + Al → Fe + Al2O3 25.9 g Fe 38.7 g

Serga [27]

<u>Answer:</u> The mass of iron produced will be 77.6 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For FeO:</u>

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

$\text{Moles of FeO}=\frac{125g}{71.8g/mol}=1.74mol$

<u>For aluminium:</u>

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{25.0g}{27g/mol}=0.93mol$

The given chemical reaction follows:

$3FeO+2Al\rightarrow 3Fe+Al_2O_3$

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = $\frac{3}{2}\times 0.93=1.395mol$ of FeO

As, given amount of FeO is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = $\frac{3}{2}\times 0.93=1.395moles$ of iron metal

Now, calculating the mass of iron metal from equation 1, we get:

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

$1.395mol=\frac{\text{Mass of iron}}{55.85g/mol}\\\\\text{Mass of iron}=(1.395mol\times 55.85g/mol)=77.6g$

Hence, the mass of iron produced will be 77.6 grams

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3 years ago

How is the nucleus of an atom split?

AnnZ [28]

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3 years ago

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stealth61 [152]

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4 years ago

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choli [55]

Answer:

False

Explanation:

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2 years ago

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