what is the pressure of 2.0 mol nitrogen (n2) gas in a 0.5 l container at 310
k?

10.304 kPa

Explanation:

n=mol nitrogen (N2) gas=2moles

Temperature=T=310 K

Volume=0.5 L=0.5 dm3

R=8.31 J K−1 mol−1

From Gerenal gas equation we know that

PV=nRT

P=nRT/V

Putting the values

P=(2*8.31*3100/(0.5)

P=10.304 kPa

or P=10304 Pa

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

answer; i believe the correct answer is (solid gold);