Question

Fe(s) + 2HNO3(aq) → H2(g) + Fe(NO3)2(aq)
If 2.34 moles of nitric acid react, what mass of hydrogen gas will be produced?

Answer 1

find the limiting reactant
2.34/2
that is the number to use for ratio
Fe will have 2.34/2 mols, nitric acid will have 2.34, hydrogen gas will have 2.34/2, iron nitrite will have 2.34/2 mols

Answer 2

i'm confused. how did you find the limiting reactant?

Answer 3

so pretty much the whole equation is a ratio.
in this case it is a 1:2:1:1 ratio.
when finding 2.34/2, this means that with one ratio of nitric acid, 1.17 mols will be created. two ratios of nitric acid is used, 2.34 will be created.

Answer 4

since nitric acid has the ratio of two but every other has one, you need to divide it by the smallest ratio

Answer 5

which is 1.17

Answer 6

this might help

Answer 7

Fe(s) + 2HNO3(aq) → H2(g) + Fe(NO3)2(aq)
Before 2.34 0
Change -2.34 +1.17
After 0 1.17

Answer 8

presuming that the reaction comes to completion of course

Answer 9

I don't understand how you got the ratio. But based on other questions, don't we need to use oxidation numbers?

Answer 10

Lol no this was how I was taught

Answer 11

Oh I just don't really understand this

Answer 12

@Tranquility I need to study lol sorry <3

Answer 13

But how do we get from mol nitric acid to hydrogen?

XD thank you for trying to help

Answer 14

AH IT ISNT FORMATTED RIGHT

Answer 15

\(\color{#0cbb34}{\text{Originally Posted by}}\) @lowkey
...............Fe(s) + 2HNO3(aq) → H2(g) + Fe(NO3)2(aq)
Before 2.34 0
Change -2.34 +1.17
After 0 1.17
\(\color{#0cbb34}{\text{End of Quote}}\)

Answer 16

okay im satisfied now bye <3

Answer 17

Welcome to QuestionCove Haley!

For every mole of Fe(s) you need 2 moles of HNO3(aq)

The limiting reactant is the reactant that runs out the first. This question doesn't involve limiting reactants though

Answer 18

Got it. That I understand now

Answer 19

so in reality, do we do what ^ said, and divide 2.34 by 2 and then convert from mol to grams?

Answer 20

Fe(s) + 2HNO3(aq) → H2(g) + Fe(NO3)2(aq)
If 2.34 moles of nitric acid react, what mass of hydrogen gas will be produced?

We have 2.34 moles of nitric acid

So for every mole of Fe(s) and 2 moles of HNO3(aq) we produce 1 mole H2(g) and 1 mole Fe(NO3)2(aq)

So if we have 2.34 moles of HNO3(aq), how many moles of H2 gas would we produce?

Answer 21

Yes, we divide by 2 because the ratio of moles between HNO3 and H2 is 2:1

So since we have 2.34 moles HNO3, we would need 2.34/2 moles of H2 gas

Answer 22

So we need 1.17mol H2 gas, so then we just need to convert that to grams?

Answer 23

Yes! Do you know how you find how many grams are in a mol?

Hint: you have to use the periodic table

Answer 24

Depends. if you were given in moles, you should give the answer in moles

Answer 25

wait ok nvm

Answer 26

But it's requesting it in grams lol

Answer 27

The question asks for grams

Answer 28

ididntseethatdontattackme

Answer 29

Isn't it 1.008 grams? since we use the atomic weight for calculations?

Answer 30

I can't remember if there are 2 or 3 zeros XD

Answer 31

so would it be \[1.17mol * \frac{ 1.008g }{ 1mol }\]

Answer 32

1.008

You need to be careful because Hydrogen's molar mass is 1.008 gram/mole

but here we're dealing with hydrogen gas which is \(\sf H_2\) so you multiply the molar mass by 2

Answer 33

oooh i forgot about that

Answer 34

so we would get 2.36 grams of hydrogen gas

Answer 35

If you are available to help, I have another similar question that I started that I need help with in another post

Answer 36

That's correct!

And sure!