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A researcher pumps 0.0128 moles of nitrogen (N2) into a 450 ml chamber held at 20 oC. What is the pressure inside the chamber?

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Answer:

Pressure inside the chamber is 0.68 atm

Explanation:

This is solved by the Ideal Gases Law:

Pressure . Volume = number of moles . R . T (in K)

T in K --> T° C + 273

20°C + 273 = 293 K

R --> Universal Constant Gas = 0.082 L.atm/mol.K

Let's replace:

P . 0.450L = 0.0128 mol .  0.082 L.atm/mol.K . 293K

P = (0.0128 mol .  0.082 L.atm/mol.K . 293K) / 0.450L

P = 0.68 atm

Be careful because you have volume in mL and you must convert to L

450 mL . 1L/1000 mL = 0.450 L

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