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lina2011 [118]
3 years ago
13

When 4.31 g of a nonelectrolyte solute is dissolved in water to make 635 mL of solution at 28 °C, the solution exerts an osmotic

pressure of 945 torr. What is the molar concentration of the solution?
Chemistry
1 answer:
blondinia [14]3 years ago
3 0

Answer:

Molar concentration is 0.050 M

Explanation:

Osmotic pressure -

Osmotic pressure is pressure applied  to stop the flow of solvent across a semipermeable membrane, from its high concentration to  its low concentration , it is a type of colligative property , i.e. , it depends on the number of moles of solute.

Osmotic pressure can be calculated from the formula -

π = CRT

π = Osmotic pressure ( in atm )

C = molarity of the solution

R = universal gas constant ( 0.082 L.atm / K.mol )

T = temperature ( Kelvin )

From the question ,

π = 945 torr

since,

760 torr = 1 atm

1 torr = 1 / 760 atm

945 torr = 1 / 760 * 945 atm

945 torr = 1.24 atm

Temperature = T = 28°C

(adding 273 To °C to convert it to K)

T = 28 + 273 = 301 K

Using the equation of osmotic pressure,

π = CRT

C = π / RT

putting the

C = 1.24 atm / 0.082 L.atm / K.mol * 301 K

C = 1.24 / 24.68

C = 0.050 M

Hence,

The Molar concentration is 0.050 M.  

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Help!!
anyanavicka [17]

I believe this a PV = nRT question whereas

you re write the formula and solve for volume

V = nRT/ P

then you input the values

P= pressure constant

V= x

n = moles = 0.2540

R = gas constant should be 8.314J mol

T = C degrees + 273.15 = K

solve for voume

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and use sig figs!!!!

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When a magnesium ribbon is heated in air the product former is heavier.on the other hand when potassium manganate(VII) is heated
vesna_86 [32]

Answer: On heating, Magnesium forms its oxide; while potassium manganate(VII) decomposes

Explanation:

Magnesium Mg, on heating forms Magnesium oxide

2Mg(s) + O2(g) --> 2MgO

Potassium permanganate KMnO4, on heating decomposes to potassium manganate K2MnO4, manganese dioxide MnO2, and Oxygen gas O2.

2KMnO4 --> K2MnO4 + MnO2 + O2

The difference in observation is that, on heating, Magnesium forms its OXIDE as product; while potassium manganate(VII) decomposes, giving OFF most of its constituents and reducing its weight.

4 0
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A compound is composed of 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen. The mystery compound has a molar mass of
vredina [299]

Answer:

C₂H₈N₄O₆ is the molecular formula for the compound

Explanation:

Data from the problem:

13 g of C in 100 g of compound

4.3 g of H in 100 g of compound

30.4 g of N in 100 g of compound

52.2 g of O in 100 g of compound

Firstly we determine, the mass of each in 184 g of compound, which is 1 mol

(13 g / 100 g) . 184 g  = 24 g C

(4.3 g  / 100 g) . 184 g  = 7.91 g H ≅ 8 g H

(30.4 g / 100 g) . 184 g  = 56 g N

(52.2 g  / 100 g) . 184 g  = 96 g O

And now, we divide the mass by the molar mass of each to determine the moles:

24 g C / 12 g/mol = 2 mol C

8g H / 1 g/mol = 8 mol H

56 g N / 14 g/mol = 4 mol N

96 g O / 16 g/mol = 6 mol O

So the molecular formula of the compound is C₂H₈N₄O₆

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