Darkblade48

I agree, as long as you know the naming system that you learned in your country of origin, then the exam is not too difficult. I remember when I took Orgo Chem 1 (and 2), there were several retrosynthesis and mechanism type problems.

Thankfully, it seems as if the equation on Wikipedia has been corrected. Of course, there is no way aqueous ammonium nitrate could decompose into nitrous oxide and water (at least not at any appreciable rate, as John Cuthber mentioned).

Try mixing a solution of hydrochloric acid with sodium hydroxide. Heat is produced as a result (amongst other things).

You can make water more conductive by simply adding ions to the solution (i.e. with sodium chloride, water becomes much more conductive); there is no need for sodium hydroxide

It is unlikely that you made any appreciable amounts of sodium hydroxide. The only danger I can see is from inhaling the ammonia fumes when you tried to boil it off.

"is a nuclear reaction reversible?"

I believe so, but the temperatures requierd are a bit awkward to deal with. Do you have a tame supernova in your lab?

Well said

Fission is certainly reversible, the reverse process is called fusion. But, as John mentioned, you'd require a tame star in your lab.

Perhaps you meant manganese dioxide? If you add it to hydrogen peroxide, it acts as a catalyst for the decomposition of the peroxide.

thanks, i'm not that smart at this

 

but wouldn't the ammonia+oxygen need to be heated to insane temperatures to oxidse? or would it react just with the oxygen being bubbled through it?

As thedarkshade mentioned, the reaction is a catalytic oxidation which requires the presence of a platinum gauze catalyst. Also, the reaction occurs at ~800 C.

What should be expected from vinegar + baking soda?

And a pool chlorine tablet + alcohol ?

If you cannot figure out the first reaction, I strongly suggest you not carry out the second!

Hydrogen peroxide often has an acid stabilizer included when it is sold over the counter, i.e. in pharmacies.

I have seen the mechanism in an introductory organic chemistry textbook (McMurry), but it's 4:10 am local time, and I don't want to be bothered looking for the mechanism (of both acid and base catalyzed decomposition) at this time....

I don't understand something; if you are trying to make ferric oxide, would it not be easier to produce it in other manners?

Oooh, a helical stair case. We have one on the university campus as well

Thanks for the wallpapers thedarkshade! Maybe it's just me, but I have a weird liking for chemistry equipment!

Sea water tastes salty due to the dissolved salts that are in sea water; a large contributing factor is the amount of dissolved sodium chloride in sea water.

Sorry to be the one to say this, but I don't think anyone will help you with your assignment unless you show that you've put some thought/effort into it.

No, I believe the stuff found in super glue is cyanoacrylate, which doesn't have a simple as structure as acetonitrile.

A quick Google search yielded:

MnO2 + 4 HCl ==> MnCl2 + 2 H2O + Cl2

I was thinking of heating the solution, because NaCl dissolves weakly in hot, so it would remain as a precipitate!

Don't heat the solution, as mentioned, this will cause the decomposition of the hypochlorite.

By cooling the solution, you will obtain a precipitate of NaCl, which can easily be filtered out, and you will be left with your hypochlorite solution.

Yes, using chlorine gas, you can bubble it through a solution of NaOH to obtain sodium hypochlorite. The reaction should be carried out in the cold in order to prevent degradation of the hypochlorite.

Yup, the final leftover product is zinc oxide (ZnO)

Anaerobic life forms (like us) have enzymes to break it down.

Did you mean aerobic life forms?

It has to do with equilibrium, actually.

Water in a closed environment (say a container), as you know, will also evaporate to some extent, but then the air becomes saturated with water moisture. The amount of water that condenses from the air to water is equal to the amount of water that evaporates from the water to the air. As a result, no more evaporation occurs.

Conversely, in an open environment, the amount of water in the air is not in equilibrium (i.e. the rate at which water goes into the air is faster than the rate at which water from the air condenses back into your beaker), so the water eventually evaporates.

Of course, if you had an air tight room, and had enough water, you could eventually saturate the air in the room so that it would be at equilibrium...

Hope that helps.

It should be once the equation is balanced, that's the point.

However, the equation given above simply doesn't make sense.

If you react those starting materials you simply cannot get those products.

There's nowhere for the chlorine to have come from.

Yes, this was my point I was trying to make. The chlorine on the right side appears from no where, and the iron and sulfur on the left disappear.

Perhaps it's just me that is missing something, but how come the conservation of matter is not followed in the equation?

I believe coke removed rust and dirt from metals due to the phosphoric acid in it.