raffle_snaffle
  • raffle_snaffle
A chemist producing ammonia by the Haber process is given 10.0 L of hydrogen gas at STP to the process a. How many moles of H2 does the chemist have? b. How many moles of N2 will the chemist require to react with H2? (use answer a.) c. How many grams of N2 will be required? d. How many liters of N2 will be required at STP (use answer b.) e. How many moles of NH3 will be produced? (use answer a.) f. How many grams of of NH3 will be produced? g. How many liters of NH3 will be produced at STP? (use answer e.)
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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jamiebookeater
  • jamiebookeater
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raffle_snaffle
  • raffle_snaffle
@Photon336
raffle_snaffle
  • raffle_snaffle
@Zale101
raffle_snaffle
  • raffle_snaffle
for a. I got 0.446 mole of H2 gas

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raffle_snaffle
  • raffle_snaffle
i am stuck on b.
raffle_snaffle
  • raffle_snaffle
i don't think I need to use pv=nrt
Zale101
  • Zale101
\(\Large N_{2(g)}+3H_{2(g)} \rightarrow 2NH_{3(g)}\) After you get the moles of H2, use mole to mole ration to find the moles for N2
Zale101
  • Zale101
mole to mole ratio*
Zale101
  • Zale101
Are you familiar with mole to mole ratio?
raffle_snaffle
  • raffle_snaffle
No not super familar can you show me plz
raffle_snaffle
  • raffle_snaffle
this isn't homework just practice
raffle_snaffle
  • raffle_snaffle
i thought when reacting H2 and N2 it is already balanced
Zale101
  • Zale101
Sure. You said you got 0.446 mole of H2 gas. We know that for every 1 mole of N2, there's 3 moles of H2. So, \( 0.446 ~mole~ H_2~\times \Large \frac{1~mole~N_2}{3~mole~H_2} \) Moles of H2 will cancel out and that will leave you with moles of N2
raffle_snaffle
  • raffle_snaffle
oh nvm about the balancing the equation I see that ammonia is stated in the problem
raffle_snaffle
  • raffle_snaffle
Okay let me look at this and study it
raffle_snaffle
  • raffle_snaffle
okay I am going to try to anser the rest myself if I have any further questions I will tag you thanks
Zale101
  • Zale101
No problem.
raffle_snaffle
  • raffle_snaffle
lol so how do we solve part c?
raffle_snaffle
  • raffle_snaffle
wait... actually let me do this
raffle_snaffle
  • raffle_snaffle
okay how do we solve part e
Zale101
  • Zale101
Okay. Question C says: c. How many grams of N2 will be required? Do you remember how to convert moles to grams?
Zale101
  • Zale101
e. How many moles of NH3 will be produced? (use answer a.) Same thing with B, you do mole to mole ratio.
raffle_snaffle
  • raffle_snaffle
i got c
Zale101
  • Zale101
There's 3 moles of H2 for every 2 moles of NH3
raffle_snaffle
  • raffle_snaffle
and d. how do we get part e using a.
raffle_snaffle
  • raffle_snaffle
okay i agree with your statement but why can't we use N2 instead of 3H2
raffle_snaffle
  • raffle_snaffle
are we going to be using a mole to mole ratio for part e?
raffle_snaffle
  • raffle_snaffle
do you know what I mean?
raffle_snaffle
  • raffle_snaffle
we are using H2 because we want to see how many moles of NH3 will be produced after the reaction?
raffle_snaffle
  • raffle_snaffle
so this is the reason we use H2 instead?
raffle_snaffle
  • raffle_snaffle
zale?
Zale101
  • Zale101
Actually, you can use whatever moles whether it's N2 or H2, but your question suggests to use answer a.
Zale101
  • Zale101
Sorry for the late reply. I was studying too.
raffle_snaffle
  • raffle_snaffle
oh okay
raffle_snaffle
  • raffle_snaffle
no problem I thought maybe you were having computer malfunctions lol
Zale101
  • Zale101
lol
raffle_snaffle
  • raffle_snaffle
h. suppose the chemist finds that they have on hand 3.00 L of nitrogen gas. Is this more or less than the amount required to react with the 10.0 L of hydrogen? i. Calculate the volume (in L) of ammonia at STP that could be produced from the 3.00 L of nitrogen in part h. j. Looking at your calculations above, determine which produces more ammonia: 10.0 L of hydrogen gas or 3.00 L of nitrogen gas ? The reactant that produces the least amount of product is called the limiting reactant for the reaction. Of course, this depends on the actual amount of each reactant you have to start with, not simply on the stoichiometry of the balanced equation.
raffle_snaffle
  • raffle_snaffle
@Zale101
Zale101
  • Zale101
At STP that translates to \(\large \frac{22.4~L}{1~mole}\)

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