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LuckyWell [14K]

3 years ago

10

Please Help ASAP! Will Mark Brainliest

2 answers:

CaHeK987 [17]3 years ago

8 0

Answer:

35. boiling point 100 Celsius

36. seven

sorry i dont know 37 AND 38. :(

Explanation:

blsea [12.9K]3 years ago

5 0

Answer: 35. it is 100°C

36. there is 7 periods in the periodic table

37. A heterogeneous mixture consists of visibly different substances or phases. ... Solutions have particles which are the size of atoms or molecules - too small to be seen. Oil and water form a heterogeneous or cereal and milk also makes a heterogeneous. a example of solution mixture is salt and water or rubbing alcohol.

38. A two phase mixture is a mixture of two different substances. An example of a two phase mixture would be a soft drink. It is a liquid and a gas. To separate these two substances you could heat the liquid and then capture the carbon dioxide.

Explanation:

I hope this helps you out buddy stay safe

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When should a lab coat, safety goggles, and gloves be worn in the laboratory?

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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

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<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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Answer:

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