The name is just scary enough... but here is my problem:
"How many kg of methane would be needed to produce 1 kg of hydrogen using the steamhydrocarbon reforming process? (Assume each step is 100% efficient.)"
The steamhydrocarbon reforming process is a three step reaction:
1. First Step At 1100 degrees C and a Ni catalyst:
H2O (g) + CH4 (g) --> CO (g) + 3H2 (g)
2. Second Step At 400 degrees C and metal oxide catalyst:
CO (g) + H2O (l) --> CO2 (g) + H2 (g)
3. No special temps or catalyst for this one:
CO2 (g) + 2OH[-] (aq) --> CO3[2-] (aq) + H2O (l)
Now, I am really lost on this one. Is this a molality problem? And if so, do I use all three reactions, just the first two, or just the first one. I tried finding a similar example of a problem like this in my book but it has been unsuccessful. The section that talks about this in my book simply gives the three reactions without explaining how to do a problem using them. All help is very much appreciated. :animatedwink: