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olga55 [171]
2 years ago
10

A 1.20 g sample of water is injected into an evacuated 5.00 l flask at 65°c. part of the water vaporizes and creates a pressure

of 187.5 mmhg. what percentage of the water vaporized?
Chemistry
1 answer:
Mkey [24]2 years ago
3 0
Assume that the water vapor is an ideal gas. So,


PV = nRT

For conversion, 760 mmHg = 101325 Pa and 1,000 L = 1 m³
(187.5 mmHg)(101325 Pa/760 mmHg)(5 L)(1 m³/1,000 L) = n(8.314 m³Pa/molK)(65+273 K)
Solving for n,
n = 0.0445 mole water

Since the molar mass of water is 18 g/mol,
Mass of water vaporized = 0.0445*18 = 0.8 g water vaporized

Hence,
Percentage of water vaporized = 0.8/1.2 * 100 =<em> 66.7%</em>
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Solve for P2 on your calculator and that should get you to the answer.


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<span>100. ppb of chcl3 in drinking water means  100 g of CHCl3 in 1,000,0000,000 g of water

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Molality, m

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mole fraction of solute, X solute

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number of moles of solution = number of moles of solute + number of moles of solvent

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number of moles of solution = 0.838 moles + 55,508,435 moles = 55,508,436 moles

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