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Alik [6]
3 years ago
9

A 50.0 mL sample of gas at 20.0 atm of pressure is compressed to 40.0 atm of pressure at constant temperature. What is the new v

olume? 0.0100 mL 0.325 mL 25.0 mL 100. mL
Chemistry
1 answer:
guapka [62]3 years ago
6 0

Ans: Final volume = 25.0 ml

<u>Given:</u>

Initial volume V1 = 50.0 ml

Initial pressure P1 = 20.0 atm

Final pressure P2 = 40.0 atm

<u>To determine:</u>

The final volume V2

<u>Explanation:</u>

Ideal gas equation: PV = nRT

under constant temperature, T and number of moles n we have:

PV = constant

or, P1V1 = P2V2

V2 = P1V1/P2 = 20*50/40 = 25 ml.

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Crazy boy [7]

Answer:

<u>5 moles S x (36.02 g S/mole S) = 180.1 grams of S</u>

Explanation:

The periodic table has mass units for every element that can be correlated with the number of atoms of that element.  The relationship is known as Avogadro's Number.  This number, 6.02x10^{23} , is nicknamed the mole, which scientists found to be a lot more catchy, and easier to write than  6.02x10^{23}.  <u>The mole is correlated to the atomic mass of that element.</u>  The atomic mass of sulfur, S, is 36.02 AMU, atomic mass units.  <u>But it can also be read as 36.02 grams/mole.</u>

<u></u>

<u>This means that 36.02 grams of S contains 1 mole (6.02x</u>10^{23}<u>) of S atoms</u>.

<u></u>

This relationship holds for all the elements.  Zinc, Zn, has an atomic mass of 65.38 AMU, so it has a "molar mass" of 65.38 grams/mole.  ^5.38 grams of Zn contains 1 mole of Zn atoms.  

And so on.

5.0 moles of Sulfur would therefore contain:

(5.0 moles S)*(36.02 grams/mole S) = <u>180.1 grams of S</u>

Note how the units cancel to leaves just grams.  The units are extremely helpful in mole calculations to insure the correct mathematical operation is done.  To find the number of moles in 70 g of S, for example, we would write:

(70g S)/(36.02 grams S/mole S) = 1.94 moles of S.  [<u>Note how the units cancel to leave just moles</u>]

4 0
2 years ago
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djverab [1.8K]

Answer:

2 sig figs.

Explanation:

Sig Fig Rules:

Any non-zero digit is a significant figure.

Any zeros between 2 non-zero digits are significant figures.

Trailing zeros after the decimal are significant figures.

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