Question

Ammonia is produced by the following reaction.


3H2(g) + N2(g) --------> 2NH3(g)


When 7.00 g of hydrogen react with 70.0 g of nitrogen, hydrogen is considered the limiting reactant because
7.5 mol of hydrogen would be needed to consume the available nitrogen.
7.5 mol of nitrogen would be needed to consume the available hydrogen.
hydrogen would produce 7.5 mol more ammonia than nitrogen.
nitrogen would produce 7.5 mol more ammonia than hydrogen.

Answer 1

find mole of both H and N

Answer 2

the one with a least mole is going to be your limiting reagent

Answer 3

hydrogen but why

Answer 4

because u have less of H in reaction
so that means the reaction will depend on amount of H

Answer 5

so whats the answer then

Answer 6

this is kinda confusing @aaronq

Answer 7

;-(

Answer 8

I have 6 questions left and 10 minutes :-(

Answer 9

only A makes sense kinda though im struggling to prove it

Answer 10

im so sorry T_T

Answer 11

its fine i entered A

Answer 12

The actual yield of the products in a reaction is always $________$ the theoretical yield.
greater than
the same as
less than
the mole ratio of

Answer 13

could u tell me what do u think?"

Answer 14

greater

Answer 15

no its actually the opposite

Answer 16

u've gotta remember that Actually yield is always less the theoretical

Answer 17

ahhhhh thank u

Answer 18

http://www.bbc.co.uk/schools/gcsebitesize/science/add_ocr_21c/chemical_synthesis/synthesisrev4.shtml
make sure to read this afterwards to understand why so, ok?

Answer 19

u r welcome :)

Answer 20

i WILL

Answer 21

omg my times running out ;-(

Answer 22

if there is any more question make sure to open a new question
and always medal the person whose answer you consider to be right/ understand/ useful

Answer 23

how do you medalsomeone

Answer 24

and Welcome to OS :)

Answer 25

i just did it

Answer 26

ok ill post my new ques

Answer 27

yeah like that
anyways lets go back to ur questions

Answer 28

okay)