Jump to content


Senior Members
  • Posts

  • Joined

  • Last visited

Posts posted by Darkblade48

  1. 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).

  2. "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.

  3. 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.

  4. 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....

  5. 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.

  6. 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.

  7. 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.

  • Create New...

Important Information

We have placed cookies on your device to help make this website better. You can adjust your cookie settings, otherwise we'll assume you're okay to continue.