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1‑propanol ( nn ‑propanol) and 2‑propanol (isopropanol) form ideal solutions in all proportions. Calculate the partial pressure and the mole fraction ( yy ) of the vapor phase of each component in equilibrium with each of the given solutions at 25 °C. P∘prop=20.9 TorrPprop°=20.9 Torr and P∘iso=45.2 TorrPiso°=45.2 Torr at 25 °C. A solution with a mole fraction of xprop=0.243xprop=0.243 .

Answers

Answer 1

Answer:

Answer:

Piso = 32.17 Torr

Pprop = 5.079 Torr

yprop = 0.1364

yiso = 0.8636

Explanation:

From the question; we can opine that :

The mole fraction of isopropanol in a mixture of isopropanol and propanol will be 1.

The partial pressure of isopropanol will be its mole fraction multiplied by vapor pressure of isopropanol

The partial pressure of propanol will be its mole fraction multiplied by vapor pressure of propanol

In the vapor, the mole fraction of propanol will be its partial pressure divided by the sum of the two partial pressures

NOW;

When xprop = 0.243; xisopropanol will be 1- 0.243 = 0.757

P°iso = 45.2 Torr at 25 °C so

Piso will be 45.2 × 0.757 = 32.17 Torr

Pprop will be 20.9 × 0.243 = 5.079 Torr

yprop = 5.079/(5.079 +32.17) = 0.1364

yiso = 1-0.1364 = 0.8636

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when the pressure that a gas exerts on a sealed container changes from 3.74 atm to ____ atm, the temperature changes from 394 K to 789 K

Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 21 ∘C∘C. Express the pressures in atmospheres to three significant digits separated by commas.

Answers

The question is incomplete, complete question is ;

A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.8 g of $O_2$ and 33.1 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 21°C.Express the pressures in atmospheres to three significant digits separated by commas.

Answer:

Partial pressure of the oxygen gas is 3.91 atm.

Partial pressure of the helium gas is 20.0 atm

Total pressure of the gases is 24.0 atm

Explanation:

Moles of oxygen gas = $n_1=(51.8)/(32 g/mol)=1.619 mol$

Moles of helium gas = $n_2=(33.1 g)/(4 g/mol)=8.275 mol$

Total moles of gas = $n_1+n_2=(1.619 +8.275 ) mole=9.894 mol$

Volume of the cylinder = V = 10.0 L

Total pressure in the cylinder = P = ?

Temperature of the gas in cylinder = T = 21°C = 21 + 273 K = 294 K

PV = nRT ( ideal gas equation )

$P=(nRT)/(V)$

$=(9.894 mol* 0.0821 atm L/mol K* 294 K)/(10.0 L)$

P = 23.88 atm ≈ 23.9

Partial pressure of the individual gas will be determined by the help of Dalton's law:

partial pressure = Total pressure × mole fraction of gas

Partial pressure of the oxygen gas

$p_(1)=P* \chi_(1)=P* (n_1)/(n_1+n_2)$

$p_1=23.88 atm* (1.619 mol)/(9.894 mol)=3.91 atm$

Partial pressure of the helium gas

$p_(2)=P* \chi_(2)=P* (n_2)/(n_1+n_2)$

$p_2=23.88 atm* (8.275 mol)/(9.894 mol)=19.97 atm\approx 20.0 atm$

Does the molarity of the solution change with the change in temperature?Match the words in the left column to the appropriate blanks in the sentences on the right.

Answers

Answer:

Yes, molarity changes according to temperature.

Explanation:

Molarity equals to moles over volume

which can be also said;

Molarity = moles of solute / liters of solution

Well, the volume or liters of the solution depends on temperature.

If the temperature is high then the volume will be higher where the molarity decreases.

Which of the following describes the change in atomic mass and atomic number during this reaction?

Answers

The mass number tells us the number (the sum of nucleons) of protons and neutrons in the nucleus of an atom. ... It is traditionally represented by the symbol Z. The atomic number uniquely identifies a chemical element. In an atom of neutral charge, atomic number is equal to the number of electrons.

The value of delta for the [C_rF_6]^3- complex is 182 kJ/mol. Calculate the expected wavelength of the absorption corresponding to promotion of an electron from the lower-energy to the higher-energy of orbital set in this complex. (Remember to divide by Avogadro's number.) Should the complex absorb in the visible range?

Answers

Answer: Yes the absorb in the visible range.

Explanation:

The relationship between wavelength and energy of the wave follows the equation:

$E=(Nhc)/(\lambda)$

where,

$E$ = energy of the wave = 182 kJ/mol = 182000 J/mol

N = avogadro's number = $6.023* 10^(23)$

h = plank constant = $6.6* 10^(-34)Js^(-1)$

c = speed of light = $3* 10^8m/s$

$\lambda$ = wavelength of the wave = ?

Putting all the values:

$182000=(6.023* 10^(23)* 6.6* 10^(-34)* 3* 10^8m/s)/(\lambda)$

$\lambda=0.65* 10^(-6)m=650nm$ $(1nm=10^(-9)m)$

The wavelength range for visible rays is 400 nm to 750 nm, thus the complex absorb in the visible range.

Final answer:

The expected wavelength of the absorption in the [CrF6]3- complex cannot be calculated without knowing the exact value of ΔE. Therefore, it is unclear if the complex will absorb in the visible range.

Explanation:

In this complex, the value of delta (Δ) is 182 kJ/mol. To calculate the expected wavelength of the absorption corresponding to the promotion of an electron from the lower-energy orbital to the higher-energy orbital, we can use the equation: Wavelength = (hc)/(ΔE), where h is Planck's constant and c is the speed of light. By substituting the given values and dividing by Avogadro's number, we can calculate the expected wavelength.

However, the information given in the question does not provide the exact value for ΔE. Without this information, it is not possible to calculate the expected wavelength accurately. Therefore, we cannot determine if the complex will absorb in the visible range.

Learn more about Calculating expected wavelength of absorption in a complex here:

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Describe the environmental impacts that are involved during the design, research and development, and marketing phases of cell phones.

Answers

Answer:

joe mama

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400 + 20 + 420

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