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3 years ago

SOMEONe HELP ME PLZ WILL MARK U AS BRAINLIEST!

Chemistry

1 answer:

leonid [27]3 years ago

8 0

Answer:

i cant see what it says

Explanation:

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What can you tell about element hydrogen

Vikki [24]

Answer:

At standard temperature and pressure, hydrogen is a colorless, odorless, tasteless, non-toxic, nonmetallic, highly combustible diatomic gas with the molecular formula H2. Since hydrogen readily forms covalent compounds with most nonmetallic elements, most of the hydrogen on Earth exists in molecular forms such as water

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3 years ago

Please help quick! Will give brainiest if you are correct!

sveticcg [70]

/the next low tide will be on monday 5th june at 2:30

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4 years ago

Which is the first step in an arson investigation that helps reconstruct the fire?

expeople1 [14]

Answer is: B. taking photographs.
Fire scene investigation begins when investigator approaches the location and start observing the scene from a distance and begin photographing. That must be done first because crowd start gathering. Once the fire scene is secured, wintesses can be interviewed.

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4 years ago

Read 2 more answers

Which type of circuit has more than one path?

Galina-37 [17]

Answer:

parallel circuit

Explanation:

Hope this is right!!

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3 years ago

You want to determine the value of x in hydrated iron II sulfate, FeSO4 xH2O. In the laboratory you weigh out 1.983 g of the hyd

jek_recluse [69]

Answer:

The value of x is 7.

Explanation:

When a hydrated salt is heated, the water evaporates because it has a lower boiling point (373 K) and what remains is the anhydrous salt (without water) The mass of the hydrated salt is equal to the sum of the anhydrous salt and the water. Since we have 2 of these 3 data, we can look for the mass of water.

mass of FeSO₄.xH₂O = mass of FeSO₄ + mass of H₂O

mass of H₂O = mass of FeSO₄.xH₂O - mass of FeSO₄

mass of H₂O = 1.983g - 1.084g = 0.899g

This means that 0.899g of water accompany 1.084 g of the salt. We want to know how many grams of water accompany 1 mol of the salt (in the molecular formula we have 1 mol of FeSO₄). Since the molar mass of is 152g/mol, we can establish:

$1mol(FeSO_{4} ).\frac{152gFeSO_{4}}{1mol(FeSO_{4} )} .\frac{0.899gH_{2}O }{1.084gFeSO_{4}} =126gH_{2}O$

As a result 1 mol of FeSO₄ is accompanied by 126 g of water. If we pass that mass into moles:

$126gH_{2}O.\frac{1molH_{2}O}{18gH_{2}O} =7molH_{2}O$

Finally, the number of moles of water in the molecular formula is x = 7.

3 0

3 years ago