A student has a 2.66 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.50 bar at 298 K . She knows that the mixture contains 0.297 mol N2 and that the partial pressure of CO2 is 0.269 bar . Calculate the partial pressure of O2 .

The partial pressure of bar.

Explanation:

Given:

Volume L

Total pressure bar

Temperature of system K

Moles of nitrogen mole

Partial pressure bar

From ideal gas equation,

Where = gas constant

First finding partial pressure of nitrogen

  bar

We know, total pressure is given by

bar

Therefore, the partial pressure of bar.

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

i don't see a text, but i am gonna assume this *orbit* the curved path, usually elliptical, described by a planet, satellite, spaceship, etc., around a celestial body, as the sun.