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storchak [24]
2 years ago
9

Glucose is a carbohydrate that contains carbon hydrogen and oxygen. The empirical formula of glucose is CH2O and it’s molar mass

is 180.12 what is the molecular formula
Chemistry
1 answer:
shtirl [24]2 years ago
6 0
Glucoses and carbonated
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A nucleus of uranium 235 decays. Its decay produces a nucleus of an unknown element (x), a nucleus of helium 4 and energy. What
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Answer: Alpha

Explanation:

Alpha particle form of decay produces a nucleus similar to the element helium. During Alpha decay an atom spits out two protons and two neutrons from its nucleus.

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2 years ago
At a certain temperature, the vapor pressure of pure benzene ‍ is atm. A solution was prepared by dissolving g of a nondissociat
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Answer:

Molar mass of solute: 300g/mol

Explanation:

<em>Vapor pressure of pure benzene: 0.930 atm</em>

<em>Assuming you dissolve 10.0 g of the non-volatile solute in 78.11g of benzene and vapour pressure of solution was found to be 0.900atm</em>

<em />

It is possible to answer this question based on Raoult's law that states vapor pressure of an ideal solution is equal to mole fraction of the solvent multiplied to pressure of pure solvent:

P_{sln} = X_{solvent}P_{solvent}^0

Moles in 78.11g of benzene are:

78.11g benzene × (1mol / 78.11g) = <em>1 mol benzene</em>

Now, mole fraction replacing in Raoult's law is:

0.900atm / 0.930atm = <em>0.9677 = moles solvent / total moles</em>.

As mole of solvent is 1:

0.9677× total moles = 1 mole benzene.

Total moles:

1.033 total moles. Moles of solute are:

1.033 moles - 1.000 moles = <em>0.0333 moles</em>.

As molar mass is the mass of a substance in 1 mole. Molar mass of the solute is:

10.0g / 0.033moles = <em>300g/mol</em>

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2 years ago
A group of students working in a chemistry lab are planning a procedure to
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use a strong base to neutralize, like NaOH, KOH, etc

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1 year ago
Free po ints<br> free po ints<br> free p oints<br> free po ints
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Answer:

thank you

thank you

thank you

thank you

Explanation:

:)

4 0
2 years ago
Read 2 more answers
HELPPPPPPPP plssss like I seriously need help
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The answer is a I’m pretty sure
8 0
2 years ago
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