A sample of air occupies 4.40 L when the pressure is 2.60 atm. (a) What volume does the sample occupy at 6.20 atm at the same temperature?

L

(b) What pressure is required in order to compress it to 0.0290 L at the same temperature?

atm

Explanation:

Given that,

Initial volume, V₁ = 4.40 L

Initial pressure, P₁ = 2.6 atm

(a) Final pressure, P₂ = 6.2 atm

As per the relation,

(b) Again using the above relation,

Hence, this is the required ssolution.

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

it would be d. henry moseley

hope this !

and sorry if i'm late. have a good rest of your day! : d