Question

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?

Answer 1

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

How do we convert mass into moles?

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

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