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?

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