When 4.96 g of a nonelectrolyte solute is dissolved in water to make 485 mL of solution at 27 °C, the solution exerts an osmotic
1 answer:
Answer:
concentration = 0.044 moles / L
Explanation:
The mass of non electrolyte solute dissolved in water =4.96 grams
The volume of water taken = 485mL = 0.485 L
the temperature = 27°C = 300 K
osmotic pressure = 827 torr =
The osmotic pressure is related to molar concentration as:
osmotic pressure = concentration X R X T
Where
R = gas constant = 0.0821 L atm/molK
Putting values
1.09 = concentration X 0.0821 X 300
concentration = 0.044 moles / L
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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, 6.02x , is nicknamed the mole, which scientists found to be a lot more catchy, and easier to write than 6.02x
. <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>
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<u>This means that 36.02 grams of S contains 1 mole (6.02x</u><u>) of S atoms</u>.
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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>]