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saw5 [17]
2 years ago
14

plz help me asap (plz don't give me helpless answer plz and ty) and also ill give brainist to the person that work hard

Chemistry
1 answer:
Vesna [10]2 years ago
8 0
Question? I don’t see anything
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Calculate the number of ammonia molecules in 3.9 g.
disa [49]
•3.9g of ammonia
•molar mass of ammonia = 17.03g/mol

1st you have to covert grams to moles by dividing the mass of ammonia with the molar mass:

(3.9 g)/ (17.03g/mol) = 0.22900763mols

Then convert the moles to molecules by multiplying it with Avogadro’s number:

Avogadro’s number: 6.022 x 10^23


0.22900763mols x (6.022 x 10^23 molecs/mol)
= 1.38 x 10^23 molecules
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What is halogens?....​
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the smallest mass of material that can sustain a chain reaction

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Critical mass refers to the smallest possible mass of a fissionable material that can sustain a chain reaction

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Consider three gases: Ar, SF6, and Cl2. If 50.0 grams of these gases are placed in each of three identical containers, which con
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The ideal gas law:
pV=nRT \Rightarrow p=\frac{nRT}{V}
p - pressure, n - number of moles, R - the gas constant, T - temperature, V - volume

The volume and temperature of all three containers are the same, so the pressure depends on the number of moles. The greater the number of moles, the higher the pressure.
The mass of gases is 50 g.

Ar \\&#10;M \approx 39.948 \ \frac{g}{mol} \\&#10;n=\frac{50 \ g}{39.948 \ \frac{g}{mol}} \approx  1.25 \ mol \\ \\&#10;SF_6 \\&#10;M \approx 146.06 \ \frac{g}{mol} \\&#10;n=\frac{50 \ g}{146.06 \ \frac{g}{mol}} \approx 0.34 \ mol \\ \\&#10;Cl_2 \\&#10;M=70.9 \ \frac{g}{mol} \\&#10;n=\frac{50 \ g}{70.9 \ \frac{g}{mol}} \approx 0.71 \ mol

The greatest number of moles is in the container with Ar, so there is the highest pressure.
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