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Sveta_85 [38]
2 years ago
12

50.0 g of nitrogen gas (N2 ) are kept under pressure in a 3.00 L container. If the pressure is kept constant, how many moles of

nitrogen gas are present in the container if gas is added until the volume has increased to 5.00 L?
Chemistry
1 answer:
kotykmax [81]2 years ago
7 0

The resultant moles of nitrogen gas that are present in the container is 2.96 moles.

<h3>How do we convert mass into moles?</h3>

Mass of any substance will be converted into moles by using the below equation as:

n = W/M, where

  • W = given mass of nitrogen gas = 50g
  • M = molar mass of nitrogen gas = 28 g/mol
  • n = 50 / 28 = 1.78 moles

From the ideal gas equation of gas we know that moles and volume is directly proportional to each other and for this question equation becomes,

V₁/n₁ = V₂/n₂, where

  • V₁ & n₁ are the initial volume and moles of gas
  • V₂ & n₂ are the final volume and moles of gas.

On putting all values, we get

n₂ = (5L)(1.78mol) / (3L) = 2.96 moles

Hence required moles of nitrogen gas are 2.96.

To know more about ideal gas equation, visit the below link:

brainly.com/question/1056445

#SPJ1

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First calculate the mole fraction of each substance:
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Raoult's Law: P(total) = P(acetone) · χ(acetone)  + P(cyclohexane) · χ(cyclohexane).
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P(total) = 185.3 torr
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