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anzhelika [568]
3 years ago
10

a sample of hydrogen gas (h2) is mixed with water vapor (h2o (g)). the make sure has a total pressure of 811 torr, and the water

vapor has a partial pressure of 12 torr. how many moles of hydrogen gas are present in a 10.0 l mixture at 298k?
Chemistry
1 answer:
Alborosie3 years ago
6 0

Answer:

n=0.430molH_2

Explanation:

Hello!

In this case, considering the partial Dalton's law of partial pressures, we can notice that the total pressure equals the pressure of steam and the pressure of hydrogen, which can be determined as shown below:

p_T=p_H+p_w\\\\p_H=811torr-12torr=799torr*\frac{1atm}{760torr}\\\\p_H=1.05atm

Thus, by using the ideal gas law, we can compute the moles of hydrogen as shown below:

PV=nRT\\\\n= \frac{PV}{RT}=\frac{1.05atm*10.0L}{0.082\frac{atm*L}{mol*K}*298K}\\\\n=0.430molH_2

Best regards!

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Answer:

The vapor pressure of the solution is 23.636 torr

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P_{solution} = X_{solvent}*P_{solvent}

Where;

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15.27 g of NaCl = [(15.27)/(58.5)]moles = 0.261 moles of NaCl

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Mole fraction of solvent (water) = (number of moles of water)/(total number of moles present in solution)

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Therefore, the vapor pressure of the solution = 0.993 * 0.0313 atm

the vapor pressure of the solution = 0.0311 atm = 23.636 torr

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