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Maurinko [17]
3 years ago
9

Biphenyl, c12h10, is a nonvolatile, nonionizing solute that is soluble in benzene, c6h6. at 25 °c, the vapor pressure of pure be

nzene is 100.84 torr. what is the vapor pressure of a solution made from dissolving 13.6 g of biphenyl in 26.4 g of benzene?
Chemistry
1 answer:
tino4ka555 [31]3 years ago
7 0
One form of Raoult's Law states that the vapor pressure of a solution of a non-volatile solute at certain temperature is equal to the vapor pressure of the pure solvent at the same temperature multiplied by the mole fraction of the solvent, this is:

p = X solvent * P pure solvent,

X solvent = number of moles of solvent / total number of moles.

Here the solute is 13.6 g of C12 H10 and the solvent is 26.4 g C6H6.

=>

moles of solvent = mass in grams / molar mass

molar mass of C6H6 = 6 * 12 g/mol + 6 * 1g/mol = 78 g/mol

moles of solvent = 26.4 g / 78 g/mol = 0.33846 mol

molar mass of C12H10 = 12 * 12g/mol + 10*1g/mol = 154 g/mol

moles of solute = 13.6 g / 154 g/mol = 0.08831 mol

=> X solvent = 0.33846 / (0.33846 + 0.08831) = 0.793

=> p = 0.793 * 100.84 torr = 79.97 torr ≈ 80.0 torr

Answer: 80.0 torr

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200.0 mL of 3.85 M HCl is added to 100.0 mL of 4.6 M barium hydroxide. The reaction goes to completion. What is the concentratio
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2.387 mol/L

Explanation:

The reaction that takes place is:

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460 mmol of Ba(OH)₂ would react completely with (2*460) 920 mmol of HCl. There are not as many mmoles of HCl so Ba(OH)₂ will remain in excess.

Now we <u>calculate how many moles of Ba(OH)₂ reacted</u>, by c<em>onverting the total number of HCl moles to Ba(OH)₂ moles</em>:

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This means the remaining Ba(OH)₂ is:

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There are two OH⁻ moles per Ba(OH)₂ mol:

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Finally we <u>divide the number of OH⁻ moles by the </u><u><em>total</em></u><u> volume</u> (100 mL + 200 mL):

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