teenwitch24
Harmless
Posts: 3
Registered: 9-2-2006
Location: Canada
Member Is Offline
Mood: No Mood
|
|
Chemistry project
Hello!
I am a student with a chemistry project. My teacher gave me an equation that I must name. I must also find a way to make the reaction go
faster. Here it is:
2Al+ 3 H2SO4? Al2 (SO4)3 + 3H2
Thanks!
Katherine
|
|
guy
National Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 982
Registered: 14-4-2004
Location: California, USA
Member Is Offline
Mood: Catalytic!
|
|
It is a single displacement reaction because Al replaces the H+. Also it could be called a redox reaction because Al reduces H+ and Al is oxidized to
Al+++. Increasing temperature by 10K usually doubles a reaction rate.
|
|
darkflame89
Hazard to Others
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 255
Registered: 1-3-2004
Location: With probability 1, "somewhere" in this
Member Is Offline
Mood: No Mood
|
|
Conversely u can also add some copper(II) sulphate to speed up the reaction too.
Ignis ubique latet, naturam amplectitur omnem.
|
|
teenwitch24
Harmless
Posts: 3
Registered: 9-2-2006
Location: Canada
Member Is Offline
Mood: No Mood
|
|
Thanks for your help, but what is it? I mean, the common name.
|
|
treelike
Harmless
Posts: 7
Registered: 6-2-2006
Location: Scotland
Member Is Offline
Mood: No Mood
|
|
Aluminium doesn't really react with sulphuric acid if I remember correctly. I guess it's one of those reactions that work in theory but when you dump
a piece of Al foil into a test tube of H2SO4 you'll see a whole lot of nothing going on.
I think the problem is that there is a film of oxide over the metal, which protects the metal from attack. If you rub some mercury over the aluminium
first this removes the oxide and I guess you could say that this will speed up the reaction, although I suspect that the oxide or possibly a sulphate
layer will build up rather quickly and slow down the reaction again.
Dump some Al into hydrochloric acid and that one is a bit more exciting, the AlCl3 produced catalyses the reaction and it gets quite violent with
hydrogen and steam coming out of the test tube (unfortunately the steam/ corrosive HCl vapour prevents the hydrogen from being ignited)
Sorry I didn't really answer the questions just blabbering for interest's sake.
|
|
neutrino
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline
Mood: oscillating
|
|
No, you're thinking of nitric acid. Sulfuric acid attacks Al just fine.
The common name? Dissolving a metal in an acid? I'm not really sure what you're looking for here.
|
|
12AX7
Post Harlot
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline
Mood: informative
|
|
Water might do it. I've distilled >92% H2SO4 + NH4NO3 (or something like that) with aluminum present in the mix and it didn't get much wear.
Seems to me moisture caused rapid corrosion (foaming and heating of the mixture).
Like iron, concentrated sulfuric has no effect on aluminum.
Tim
|
|
neutrino
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline
Mood: oscillating
|
|
Really? I didn't know that. I thought that concentrated sulfuric acid's strong oxidizing properties only became significant at high temperatures, such
as when dissolving silver.
|
|
teenwitch24
Harmless
Posts: 3
Registered: 9-2-2006
Location: Canada
Member Is Offline
Mood: No Mood
|
|
Thanks for your help, I just want to check if I got it right. A metal and an acid produce a gaz? Wich is hydrogen. To make the reaction go faster, I
simply need to heat it up?
|
|
sparkgap
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1234
Registered: 16-1-2005
Location: not where you think
Member Is Offline
Mood: chaotropic
|
|
For reactions like that, yes. Heat has this nice tendency to increase the so-called "rate of reaction"... ![;)](./images/smilies/wink.gif)
sparky (^_^)
"What's UTFSE? I keep hearing about it, but I can't be arsed to search for the answer..."
|
|
runlabrun
Hazard to Others
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 172
Registered: 4-12-2004
Member Is Offline
Mood: No Mood
|
|
in schools sometimes these reactions are generalised to be 'hydrogen producing reactions' seeing as the reaction of any metal and acid produces
hydrogen. However doesnt NaOH and Al make hydrogen too?
As a teacher i see this going on all the time in schools, teachers who may not be fully qualified in chemistry rather being allowed to teach chemistry
due to a few subjects or inservice training sessions they have attended (bad i know but it does happen) are usually the culprits. I personally dispise
these common terms being used to describe such reactions as they are not appropriate chemical descriptors of exactly what is going on, hence the
students get no real benefit except confusion.
So as for general terms i would say the teacher is asking for this... either metal/acid reaction or hydrogen producing reaction. As for speeding it
up, increase catalyst - temp is an obvious one...
@darkflame89
how does CuSO4 spead up this reaction? wouldnt sulfate solubility in conc H2SO4 would be low due to common ion interferance?
-rlr
|
|
woelen
Super Administrator
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 7998
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
CuSO4 does not speed up this reaction. A combination of CuSO4 and NaCl (or CuCl2 alone), however, tremendously speeds up the reaction. If only NaCl is
added then again there is no speed up.
The combination of Cu(2+) ion, Cl(-) ion and acid is extremely powerful in dissolving Al-metal, MUCH more than acid alone. Try it and you'll
be surprised.
|
|
tom haggen
Hazard to Others
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 488
Registered: 29-11-2003
Location: PNW
Member Is Offline
Mood: a better mood
|
|
Quote: |
hence the students get no real benefit except confusion.
|
Am I to assume that confusion is considered a benefit?![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif) ![:P](./images/smilies/tongue.gif)
N/A
|
|
darkflame89
Hazard to Others
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 255
Registered: 1-3-2004
Location: With probability 1, "somewhere" in this
Member Is Offline
Mood: No Mood
|
|
CuSO4 would speed up the reaction, just very slightly. I did an experiment once in school, where we timed the rate of reaction of magnesium reacting
with sulphuric acid. As a separate reaction, 2 drops of CuSO4 was added. The rate of reaction was higher after adding the CuSO4. This is because of a
side reaction: Mg + Cu(2+)---->Mg(2+) + Cu. The formed copper metal on the magnesium then forms a electro-couple. This causes the magnesium to
react with the acid much faster. This is very much like inserting an iron bar halfway in to an acid solution. At first, there are very little bubbles
on it, i.e. rate of reaction is slow. Place another bar of copper metal into the acid and connect the iron bar to the copper bar by means of wire.
Hydrogen will start to evolve at the copper bar at a much faster rate, and iron would rapidly dissolve in the acid.
Of course in this case, just copper sulphate is not enough to catalyse the reaction between aluminium and acid. This is due to the aluminium oxde
layer on top of the aluminium which very much stops the reaction. Even copper sulphate does not react with passivated aluminium. As Woelen pointed
out, using copper(II) chloride instead may have a greater result. The rate of reaction is so fast that in certain instances, the water may actually
boil. (No joke, i tried it once, and accidentally touched the sides of the beaker. I ended up scalded.)
Ignis ubique latet, naturam amplectitur omnem.
|
|