Question

Consider the following chemical reaction:
C(s)+H2O(g)→CO(g)+H2(g)
How many liters of hydrogen gas is formed from the complete reaction of 14.2g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360K.

Answer 1

mass of C (given)
-> mass of H2O
-> mass of H
-> mass of H2
-> volume of H2 (ideal gas law)

Answer 2

No. of C moles=14.2/12=1.18 mol
no. of H2 moles = 1.18 mol
pv=nRT
n=pv/RT
1.18=1*V/0.082*360
V= 34.932 L

Answer 3

(Forgive me if I made any mistake, I'm not a pro in Chemistry) Can you please explain it to me? I also want to learn :)

Answer 4

Tell me your problem

Answer 5

Well, is my approach wrong?

Answer 6

How did you get 1.18 mol of H2? I think that's where I went wrong when I tried working it out.

Answer 7

after finding C moles we can directly say No. of H2 moles through stoichiometry.C : H2 = 1 ; 1 and then use ideal gas law

Answer 8

Is there a problem?

Answer 9

Why C:H2=1:1?

Answer 10

C(s)+H2O(g)→CO(g)+H2(g)

if 1mol of C reacts with H20 1 mol of H2 is produced according to the reaction.So the ratio
between C and H2 is 1: 1

Answer 11

Ohh! Thank you!!

Answer 12

Oh, thanks, I'm learning Chemistry by myself

Answer 13

Thanks so much :D

Answer 14

That's exactly what you should do. Don't give up.

Answer 15

Kc, like you, I'm learning chem on my own also. This forum is a major help! Love it! :)