Which gas diffuses faster, NH3 or NO2? How many times faster?
613443
Niuchemist is mostly right and deserves the vote, but there is one correction I would make-heavier molecules don't necessarily have less "kinetic energy", they move more slowly-it is the speed of movement that is the critical thing, not the kinetic energy, which is a product of speed *and* mass.
1117190
Five feet per second.\n\nSeriously, it depends on a lot of different conditions.  Smells travel in the air by what's called diffusion. Molecules are always moving, bumping and jostling each other, so they mix. The rate of natural mixing or diffusion depends on how often molecules encounter one another. The same with how long it takes a smell to dissipate. If the wind is blowing, there will be more mixing. That can either make the smell reach you sooner, or it can spread the smell out so that you don't notice it at all. \n\nThe speed with which a smell travels depends on how fast the molecules are going, how massive they are, the relative temperature of the molecules making the smell, and how many molecules there are in a given volume, their density. We express all this mathematically as a gas's temperature and pressure. By the way, our brains are quite used to air, so for the most part, we don't smell oxygen, nitrogen, or carbon dioxide; we smell the other molecules instead.
193517
You don't provide enough data to determine this.  The gas law PV=nRT has variables you need to define.
518629
not too much, they are both basic, and don't really react. even if it is an aqueous solution of ammonia (thus avoiding the gas problem above)
497226
2NH4V03 + H2S04 ---> (NH4)2S04 + 2V02 + H20
968707
NH3  -33.34 °C\nCH3F -78°C\nCH4 −161.6 °C\nHe -268.93 °C
241737
The rate at which gases diffuse is inversely proportional to the square root of their densities. \n\nSince volumes of different gases contain the same number of particles (see Avogadro's Hypothesis), the number of moles per liter at a given T and P is constant.  Therefore, the density of a gas is directly proportional to its molar mass (MM).
946720
I think hydrogen will move faster because Mr of hydrogen molecule is smaller than that of oxygen molecules.
813106
Just an initial note: NH3 is ammonia\n\nA. \nInitial math:\nSince you have 8.5 grams of NH3, you have to convert grams mols, then into molecules. \nSo you do: 8.5 grams of NH3 / 17 grams in 1 mole of NH3 and X 6.022 x 10^23 molecules in one mole\nYou get 3.011 x 10 23 molecules, and from that you subtract 1.5 x 10^23 molecules, and you get: \n<b>1.511 x 10^23</b>\n\nB. Then, you convert 1.5 x 10^23 to moles by dividing by 6.022 x 10^23 moles, which equals .249 moles of NH3. \nThen you convert 8.5 grams of NH3 to moles too by dividing 17 grams of NH3 per mole again, and get: .5 moles! \nso: .5 mol - .249 mol = <b>.241 mol</b>\n\nC. \nFrom before, you know 1.5 x 10^23 molecules of NH3 is .249 moles. You convert this to grams by multiplying .249 by 17 grams per mol and get: 4.233 grams. \nSo: 8.5 grams - 4.233 grams = <b>4.267 grams</b>\n\nD. From before, you know you have .241 moles of ammonia left. So, you multiply this by avocado's number (6.022 x 10^23) and get: 1.45 x 10^23 molecules of ammonia. Then, you can see that there are 3 atoms of hydrogen of per molecule of ammonia, and multiply the number of molecules by 3 and get: \n<b> 4.354 x 10^23</b> \n\nI think those should be right. Sorry about the sig figs though!
424662
the fumes of HCl and NH3 react and form NH4Cl
766259
4 NH3 + 3 O2 ---> 2 N2 + 6 H20
716053
in NH3 , N is -3, each H is +1\n\nin NO2- N is +3     each O is -2\n\nin NO3- N is +5, each O is-2
211111
Two things make a difference here. The average distance that an individual particle is likely to move before it bangs into another particle and the speed at which the particles are moving.\n\nBecause the space between particles is so much larger in a gas than in a liquid at the same temperature, the "free path length" is longer in a gas and the diffusing substance is typically able to move further in a given period of time.  Therefore, gases diffuse through gases much more rapidly than liquids through liquids if all else is equal.\n\nFor any given combination, the hot gas or liquid substrate will provide more rapid diffusion compared to the cold one due to particle speed.\n\nYou need to check out Graham's Law of Diffusion if you want to get mathematical about this.
663581
NH4NO2 --------------> N2 + 2H20 \n\nYOU NEED TO HEAT THE SOLUTION IN ORDER TO DECOMPOSE THE COMPOUND \n \nHOPE THIS HELPS
839197
Nitrogen by far. it is approximately 78% of what we are breathing
251099
F.W. of CHCl3 = 119.39g\n\nF.W. of Ne = 20.18g\n\neffuses rate of  CHCl3 :\n\n square root of (20.18g / 119.39g) = .411 times as fast as Ne
314441
The chemical compound ammonium nitrate\nNH4 NO3