Inorganic Chemistry

So, here's my problem. Calculate how much HNO3 you can get (theoretically) from 1000 cubic meters of NH3. Now, the only way of getting HNO3 using NH3 is this one: 4NH3 + 5O2 -> 4NO + 6H20 2NO + O2 -> 2NO2 3NO2 + H2O -> 2HNO3 + NO So I thought I could do it this way: from 4NH3 I get -> 2 HNO3 so, from 89,6 cubic dm of NH3 I get -> 126,0256g of HNO3 then, from 1.000.000 cubic dm of NH3 I will get -> x (unknown mass) of HNO3 But the problem is, I get the wrong result when I calculate it. I get 1.406, 53 kg and the solution at the end of t…

The problem is this: Calculate how much heat is being released in the reaction of white phosphorus turning into red phosphorus if the mass of white phosphorus is 1000 kg. Standard enthalphy of this reaction is -16,73 kJ/mol. Now, I tried solving it using proportion, like this: P4 -> Pn 123,89g ... -16,73kJ 1.000.000g ... x But when I calculate x, I get 135.033,6543 kJ, and the solution at the back of the book is different, it's 5,4 * 10^5 kJ. Can someone please tell me where I made mistakes? Thanks.

Hi, I remember performing a practical once whereby ammonia solution was added to a solution of Nickel(II) chloride, with a purple precipitate appearing. This has always stuck with me as an example of an insoluble complex, and noting that many other ammonia complexes are soluble, it has now got me wondering why some complexes of any kind dissolve whilst others don't. Could anyone who has more theory please recommend to me something which would help me understand why some complexes dissolve and others don't in water under standard conditions? I realise this may be a bit involved, so I was thinking of a textbook or an area of inorganic chemistry which covers this? Many thank…

Does a chemical reaction proceed from low pKa to high pKa or high pKa to low pKa? A large Ka implies how readily a reaction goes toward the products. Now since pKa=-log(Ka), wouldn't that imply that a chemcial reaction goes from high pKa to low pKa?

I need some help with this please :why the OCCl2 does not have resonance? how to know if a compound has resonance or not ?

some experiments require an inert atmosphere. does anybody know how one can be achieved at home easily?

Effective Nuclear Charge (Zeff) is defined as how tightly the valence e- are held. I understand that Zeff decreases down a group because there is an increase in the number of principle energy levels (PEL) and as such, the valence e- are further away from the nucleus. However, Zeff increases left to right across a period. I am trying to understand this, but am having a difficult time. I understand that the number of protons and e- increase across a period, but how is that conducive to a tighter attraction with the nucleus? Thanks.

Elements on the periodic table get both oxidized and reduced. The elements that tend to get reduced are the ones closer as you go to to the right of the periodic table. Reduction is defined as an element gaining electrons. As reduction increases from right to left, IE also increases because the elements want to hang on to their electrons. Now electron affinity (EA) is the energy of an atom to gain an electron. Elements want to have an octet and so they want to gain electron, but how is that it takes more energy to gain an electron, if gaining an electron makes the element more stable? At the same time, Lewis bases are classified as electron pair donors. What does not make…

Well, I was bored one day two years back, and had just started collecting the elements of the Periodic Table. I read up on as many as I could, to get a better sense of how to make each one if possible. Then, as my head slowly became crammed with knowledge, I found I needed a place to put it all down so I could remember it. Thus, this guide was born. Before you start reading it, however, be sure to read the following. -If you know a simpler method of getting an element (other than buying it outright from a chemical supplier), then by all means, tell me! -Quite a few radioactive elements are discussed here, so if you're the kind of person who instantly gets chills up t…

I am curious about the properties of neon in it's liquid state. More precisely does it dissolve other elements and chemicals? Specifically I was wondering about liquid neon at about 10 bar and would it dissolve water? I know what water is an ice at liquid neon temps even at 10 bar but many solids dissolve in liquids, would neon dissolve water ice and if it would how easy would this happen, also would the pressure significantly influence it's ability to dissolve other chemicals? Or is neon unlikely to dissolve anything due to being a noble element?

Either today or later this week I will be receiving 60 grams of Gallium to add to my collection. Right now, I have my meager amount of gallium in a 20 mL vial as a solidified blob. My 60 grams of Ga will be arriving as two 30 gram buttons. So my task will be to melt the Ga and pour it into the glass vial where I will need to resolidify it. The problem is, Ga expands as it freezes so if I freeze it too quickly it may crack the glass vial. I'm pretty sure that it won't crack, however, since there will be plenty of room for it to expand upward if it needs to. (It's like a bottle of soda. A full bottle of soda will explode if it freezes because the liquid inside will e…

hi friends, i need your help in chemical reaction,making boron trichloride but one very toxic byproduct gas is created hence want to take all precautions When Arsenic trichloride is reacted with Sodium Borohydride it is reduced to Arsine gas and Boron trichloride. my question is, 1.Does any catalyst needed for this reacion? 2.Does this reduction do not need heating? 3.Arsenic Trichloride is liquid at RM,is this reaction is spontaneous? I searched many books but havent found answers to above.

I just recently got selenium for my element collection but I'm afraid to take it out of the bag because I've heard about selenium toxicity. I know its deadly if you ingest it but is it OK to touch it?

So, after a few months of heavy research, I came up with this: Lanthanum (La) To obtain Lanthanum, see the process for Cerium. Cerium (Ce) Metallic cerium is found in 50% or higherconcentrations in magnesium firestarters, known as “mischmetal” flints. To getthe cerium, you must first obtain a bunch of mischmetal parts. To heat it to just the righttemperature, I would suggest a Bunsen burner, which burns at about 900 degreesC, perfect for this application. Use a steel crucible, preferably with asupermagnet attached to it (so that the iron oxide draws to here). When the ceriumis liquid, and there is something floating on top, scoop it out and separateany iron …

hey, i wanted to collect chlorine gas at home, by electrolysing sodium chloride. anybody know a simple way of doing this. also i want to try to get copper metal into ions because they look really awesome. however i am at home and dont have any acid, so if anyone could sugget a way to do this, it would really help.

Okay so I'm only age 17 and am looking to major in chemistry. I love my chemistry class I'm in but unfortunately my teacher hasn't really noticed my interests towards chemistry, so I have came here for some advice, tips or anything else a beginning chemist could benefit from, I would also like to know if there is any good literature out there for newbies. I also have a few questions regarding some rather complex (imo) compounds. The first question is Ceasium Hydroxide how caustic is it exactly? Has anyone here worked with it? The second question is how safe is it to mix super small amounts of bleach and ammonia outside? (I would just like to observe the chlorine gas)…

Hey there - I was searching the net for ways to synthesize concentrated nitric acid (98%). The only methods I have come across so far have been synthesis by 98% Sulfuric Acid and some plastic sheet that can stand hot HN03, a 1000 ml beaker, a caculated amount of nitrate, and a 100ml beaker. You have to keep the beaker in the middle of the big beaker, and pour nitrate and the H2S04 mix around the small beaker and put the platsic foil over the whole thing and make sure it bulges in a bit and then lit it hang over the little beakers in the middle and it then hast to be secured with a rubber band and then it should be filled with ice water. After heat is given by a hot pla…

Used to get a few laughs painting this stuff on door handles occasionally. But I have never known exactly what compound you get when you disolve iodine in 880 ammonia. Can anyone enlighten me?

I'm not sure if this is in the right forum, but it's not a homework problem, so I thought I'd ask it here. This may be an obvious answer that I'm overlooking, but I'm curious. In the case of a complex such as [Ru(phen)2(qdppz)]2+, I KNOW that qdppz (quinone phased dipyridophenazine) is the intercalating ligand, but I don't know why. Why does qdppz intercalate and not the phen ligand? Thanks!

hello, i'm looking for a few compounds that will help me create a shower melt (substance melts at bathroom shower temperatures) without using organic materials. they need to be non-toxic and non slippery as well. can someone throw some ideas my way? any information would be helpful. TIA.

I am not sure I believe it! Hydrogen gas can be liberated by partial oxidation of formaldehyde using either H2O2 or CuO under certain reaction conditions. Journal of the Society of Chemical Industry, Volume 18, p716-717. [July 31, 1839] The fact that hydrogen and oxygen gas can be liberated together from the same solution simultaneously may also be of interest, for making gas explosions inside of closed plastic bottles.

So if I have something like NaCl and put it in water, NaCl becomes an aqueous solutio. But in an aqueous solution, the ionic equation for salt is Na+1 and Cl-1 since the ions are surrounded by water molecules. But if the ions aren't actually together and they are surrounded by water, why doesn't salt explode to produce sodium hydroxide if sodium is by itself? Why would a solution also taste salty still? Should't it taste like burning metal and bleach mixed together?

hello every one i need some help about the symmetry of crystals i cant understand it i need help

I was thinking about what possible routes there might be to potentially making sulfur diiodide, since this simple compound is apparently so elusive. I imagine researchers have already attempted all the obvious routes. What about reacting excess anhydrous hydrogen iodide with SF4 ? The only fluroide of iodine that can be isolated is iodine pentafluoride. Presumably SF4 would not oxidize I2. SF4 + (4)HI --> SI2 + I2 + (4)HF The iodine could potentially ionize in the form of H2F[+] I[-], which could be problematic. Best to use at least 8 equivalents of HI for every 1 SF4. What do you think would this work? Other typical routes, such as SH2 with io…

Hey Everyone. What is copper phosphate soluble in? I've read that it's insoluble in water...