Stoichiometry problem

  • Thread starter lolecules
  • Start date
  • #1
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Homework Statement



"How many grams of hydrogen are necessary to react completely with 50.0g of nitrogen in the below reaction?"

Homework Equations



N2+3H3 ---> 2NH3


The Attempt at a Solution



16.1g H?
 

Answers and Replies

  • #2
1,753
1
Show your work.
 
  • #3
5
0
50gN/1 1molN/28gN 3molH/1mol N 3gH/1molH
 
  • #4
1,753
1
50gN/1 1molN/28gN 3molH/1mol N 3gH/1molH
Close enough, I didn't round off like you did.
 
  • #5
5
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I guess my only question is since N2 is diatomic, then the molar mass of the nitrogen goes from 14 to 28?
 
  • #6
1,753
1
I guess my only question is since N2 is diatomic, then the molar mass of the nitrogen goes from 14 to 28?
That's right.
 
  • #7
5
0
3gH/1molH
Um, so would that also mean here the molar mass of should be changed to 6...so the answer would be 32.14g?
 
  • #8
1,753
1
Dangit, after looking at your problem. I didn't even notice you messed up the reaction equation. It's Hydrogen gas, [tex]H_2[/tex], not [tex]H_3[/tex]. Fix that and it's solved.
 
  • #9
93
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Roco, are you slipping? :)
 
  • #10
5
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Sorry for bringing up a dead topic, but I didnt want to just start a new one for basically the same thing...I just wanted to ask...

5 L N2/1 1molN2/22.4L N2

That's how I began setting up a problem, but is 22.4 right? Should it be something different since Nitrogen is diatomic?
 
  • #11
119
0
The volume of one mol of any gas at standard temp/pressure is 22.4 I don't care if it's gaseous Uranium.

22.4
 

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