Question

In the Haber process nirtrogen reacts with hydrogen to give ammonia. What is the theoretical yield of ammonia in grams that can be prepared from 41.0 g of nitrogen and excess hydrogen? Steps please

Answer 1

step one, write a balanced equation

Answer 2

step two, take 41.0g N and covert it to ammonia produced. that should be your theoretical yield

Answer 3

Thanks! I have done that multiple times and have always gotten 52 (rounded), do you get the same result?

Answer 4

whats your balanced eqn

Answer 5

N2+ 4H2 --> 2NH4

Answer 6

i think its just N+3H=NH3

Answer 7

nh4 is ammonium

Answer 8

49.8gNH3

Answer 9

OOOOh. lol Wow. Facepalm.

Answer 10

yeah that question was confusing

Answer 11

H2 would be hydrogen gas

Answer 12

and N2 nitrogen gas

Answer 13

Oh I see, been a while since I have learned chem.

Answer 14

diatomic molecues such as h2 and n2 are the result of evaporation or heating

Answer 15

but if it doesnt say that in the problem you should have to worry about that

Answer 16

Im doing something wrong i think... I got 3.02 g

Answer 17

start with 41.0g N

Answer 18

convert to moles, multiply by the mole N to mole NH3 ratio (1:1 in this prob)

Answer 19

then convert mole NH3 to grams NH3

Answer 20

41 g N x 1 mol N/ 14.007 g N x 1/1

Answer 21

x 17.0307 g NH3/ 1mol NH3 right?

Answer 22

yes

Answer 23

so 49.85 g NH3 is my theoretical yeild

Answer 24

*yield

Answer 25

yeah thats what i got

Answer 26

Awesome. Thanks a lot man! That whole gas non gas thing can really mess up on a test/ quiz. I should study basics more. haha. *fanned :)

Answer 27

no prob! goodluck! and don't worry im still learning the basics also. google helps me a lot. lol