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Andru [333]
3 years ago
6

At 293 K, methanol has a vapor pressure of 97.7 Torr and ethanol has a vapor pressure of 44.6 Torr. What would be the vapor pres

sure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K?
Chemistry
1 answer:
Bad White [126]3 years ago
8 0

Answer: The vapor pressure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K is 78.3 torr.

Explanation:

According to Raoult's law, the vapor pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the vapor pressure of that component in the pure state.

p_1=x_1p_1^0 and p_2=x_2P_2^0

where, x = mole fraction in solution  

p^0 = pressure in the pure state

According to Dalton's law, the total pressure is the sum of individual pressures.

p_{total}=p_1+p_2p_{total}=x_Ap_A^0+x_BP_B^0

moles of ethanol=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{80g}{46g/mol}=1.7moles

moles of methanol= \frac{\text{Given mass}}{\text {Molar mass}}=\frac{97g}{32g/mol}=3.0moles

Total moles = moles of ethanol + moles of methanol = 1.7 +3.0 = 4.7

x_{ethanol}=\frac{1.7}{4.7}=0.36,

x_{methanol}=1-x_{ethanol}=1-0.36=0.64

p_{ethanol}^0=44.6torr

p_{methanol}^0=97.7torr

p_{total}=0.36\times 44.6+0.64\times 97.7=78.3torr

Thus the vapor pressure of a mixture of 80 g of ethanol and 97 g of methanol at 293 K is 78.3 torr.

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Which analogy can best be likened to the activation energy of a chemical reaction?
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6 0
3 years ago
There is about 1.0 g of calcium as Ca2+ in 1.0 L of milk. What is the molarity of Ca2+ in milk?
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Explanation:

It is known that molarity is the number of moles present in a liter of solution.

           Molarity = \frac{\text{no. of moles}}{volume}

Also, number of moles equal mass divided by molar mass. And, molar mass of calcium is 40.07 g/mol.

               No. of moles = \frac{mass}{\text{molar mass}}

                                     = \frac{1.0 g}{40.07 g/mol}

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Therefore, calculate the molarity as follows.

             Molarity = \frac{\text{no. of moles}}{volume}

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7 0
3 years ago
Determine the number of atoms in 5.88 moles sodium.
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4 0
3 years ago
The partial pressure of CH4 is 0.175 atm and that of O2 is 0.250 atm in a mixture of the two gases. What is the mole fraction of
tresset_1 [31]

Answer:

The total number of moles of gas in the mixture is 0.16939.

1.25550 grams of methane gas and 3.18848 grams of oxygen gas.

Explanation:

Total volume of the mixture = V = 10.5 L

Temperature of the mixture = T = 35°C = 308.15K

Pressure of the mixture = P

Total moles of mixture = n =n_1+n_2

Using an ideal gas equation :

PV=nRT

P\times 10.0 L=n\times 0.0821 atm L/mol K\times 308.15 K

P=2.509 n

Partial pressure of the methane= p_1=0.175 atm

Moles of the methane= n_1

Partial pressure of the oxygen gas= p_2=0.250 atm

Moles of the methane= n_2

Mole fraction  of the methane= \chi_1=\frac{n_1}{n_1+n_2}

Mole fraction  of the oxygen gas= \chi_2=\frac{n_2}{n_1+n_2}

p_1=p\times \chi_1  (Dalton's law)

0.175 atm=P\times \frac{n_1}{n_1+n_2}

0.175 atm=(2.509 n)\times \frac{n_1}{n}

n_1=0.06975 mol

Mass of 0.06975 moles of methane gas :

0.06975 mol × 18 g/mol =1.25550 g

p_2=p\times \chi_2  (Dalton's law)

0.250 atm=P\times \frac{n_2}{n_1+n_2}

0.250 atm=(2.509 n)\times \frac{n_2}{n}

n_2=0.09964 mol

Mass of 0.06975 moles of oxygen gas :

0.09964 mol × 32 g/mol =3.18848 g

Total moles of mixture = n =n_1+n_2

[/tex]=0.06975 mol+0.09964 mol=0.16939 mol[/tex]

7 0
3 years ago
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