# Stoichiometry problem

1. Feb 10, 2008

### lolecules

1. The problem statement, all variables and given/known data

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

2. Relevant equations

N2+3H3 ---> 2NH3

3. The attempt at a solution

16.1g H?

2. Feb 10, 2008

### rocomath

3. Feb 10, 2008

### lolecules

50gN/1 1molN/28gN 3molH/1mol N 3gH/1molH

4. Feb 10, 2008

### rocomath

Close enough, I didn't round off like you did.

5. Feb 10, 2008

### lolecules

I guess my only question is since N2 is diatomic, then the molar mass of the nitrogen goes from 14 to 28?

6. Feb 10, 2008

### rocomath

That's right.

7. Feb 10, 2008

### lolecules

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. Feb 10, 2008

### rocomath

Dangit, after looking at your problem. I didn't even notice you messed up the reaction equation. It's Hydrogen gas, $$H_2$$, not $$H_3$$. Fix that and it's solved.

9. Feb 11, 2008

### MichaelXY

Roco, are you slipping? :)

10. Feb 11, 2008

### lolecules

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. Feb 11, 2008

### Riogho

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