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4 years ago

1. What causes water's low vapor pressure? (1 point)

1 answer:

5 0

<span>1. What causes water's low vapor pressure? (1 point)
dispersion forces
dispersion forces
covalent bonding
hydrogen bonding
ionic attractions
2. Which of the following substances is the most soluble in water? (1 point)
sodium chloride
methane
bromine
carbon
3. Which of the following substances is NOT an electrolyte? (1 point)
KCl
CCl4
LiCl
Na2SO4
4. Which of the following mixture types can be filtered to remove solute? (1 point)
suspensions only
colloids only
suspensions and colloids
suspensions and solutions
5. Which of the following mixtures is NOT a colloid? (1 point)
fog
milk
paint
sugar water
6. Which of the following types of mixtures exhibit the Tyndall effect? (1 point)
suspensions and colloids
suspensions and solutions
colloids and solutions
colloids only
7. An emulsyfying agent is typically characterized by having ____. (1 point)
one polar end
one nonpolar end
one nonpolar end
two polar ends
one polar end and one nonpolar end</span>

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2. How is the solute being dissolved in the given solvent?

galben [10]

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3 years ago

PLZ HELP "NO LINKS"

Natalka [10]

Answer: (a) Mole fraction of $H_{2}$ is 0.66.

Mole fraction of $N_{2}$ is 0.33

(b) The partial pressure of $H_{2}$ is 1.98 atm.

The partial pressure of $N_{2}$ is 0.99 atm.

(c) The total pressure is 3.0 atm

Explanation:

Given: Volume = $22.4 dm^{3}$ (1 $dm^{3}$ = 1 L) = 22.4 L

Moles of $H_{2}$ = 2.0 mol

Moles of $N_{2}$ = 1.0 mol

Total moles = (2.0 + 1.0) mol = 3.0 mol

Temperature = 273.15 K

Now, using ideal gas equation the total pressure is calculated as follows.

$PV = nRT\\$

where,

P = pressure

V = volume

n = number of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$PV = nRT\\P \times 22.4 L = 3.0 mol \times 0.0821 L atm/mol K \times 273.15 K\\P = 3.0 atm$

The mole fractions of each component:

The mole fraction of $H_{2}$ is calculated as follows.

$Mole fraction = \frac{moles of H_{2}}{moles of H_{2} + moles of N_{2}}\\= \frac{2.0 mol}{(2.0 + 1.0) mol}\\= 0.66$

The mole fraction of $N_{2}$ is as follows.

$Mole fraction = \frac{moles of N_{2}}{moles of H_{2} + moles of N_{2}}\\= \frac{1.0 mol}{(2.0 + 1.0) mol}\\= 0.33$

The partial pressures of each component:

Partial pressure of $H_{2}$ are as follows.

$P_{H_{2}} = P_{total} \times mole fraction of H_{2}\\= 3.0 atm \times 0.66\\= 1.98 atm$

Partial pressure of $N_{2}$ are as follows.

$P_{N_{2}} = P_{total} \times mola fraction of N_{2}\\= 3.0 atm \times 0.33\\= 0.99 atm$

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Identify the types of chemical reactions occurring in the chemical Quetion‘s.

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In this reaction one reactant is decomposed into two or more products

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In this reaction higher reactive element displaces lower reactive element from its solution

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3 years ago

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