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3 years ago

7

A sample of nitrogen gas has a volume of 578 mL and a pressure of 124.1 kPa. What volume would the gas occupy at 80.2 kPa if the

temperature remains constant?

1 answer:

Nataly_w [17]3 years ago

4 0

Answer:

V2 = 894.4mL

Explanation:

P1= 124.1, V1= 578mL, P2 = 80.2kPa, V2= ?

Applying Boyle's law

P1V1 = P2V2

Substitute and simplify

124.1*578=80.2*V2

V2= 894.4mL

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Determine the partial pressure and number of moles of each gas in a 15.75-L vessel at 30.0 C containing a mixture of xenon and n

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Answer:

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Explanation:

Let the total pressure of the vessel= 6.5 atm and mole fraction of Xenon= 0.761

As we know,

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According to Dalton's Law of partial pressure-

$P_i=\chi_i\times P_{total}$

Where,

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$P_t=$ The total pressure of the mixture

$P_{Xe}=(0.761)\times(6.5)\\P_{Xe}= 4.95 atm\\\\\\P_{Ne}=(0.239)\imes (6.5)\\P_{Ne}= 1.55 atm$

<u>Calculation: </u>

To calculate the number of moles,

PV=nRT

$n=\frac{PV}{RT}$

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Learn more about Dalton's Law of partial pressure here;

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