The solubility of I2 in H2O is 0.030 g/100 mL at 25°C; its solubility in carbon disulfide, CS2,?
352290
a) 0.03/200 = 3/2000\n\nno because grams are good enough and the zero's move about to make it work anyway.\n\nb) 3/2000 * 0.03 =4.5e-5g\n\nc) 3/2000 * 4.5e-5 = 6.75e-8\n\nd) method c since the carbon sulphide is no where near saturation you can split it up into smaller portions and extract far more iodine.
937928
Iodomethane CH3I has a relative molecular mass of 142 ( C = 12;  +  H3 = 3  +  I  =  127)\nIodomethane is a liquid.\nIt is dense (because of the iodine) 2.28 times heavier than water\nIt has a boiling point of 42C\n\nHalf the volume of calcium hydroxide would be needed because it is dibasic ( has two OH groups)\n\n  Ca(OH)2  +   2HCl  =   CaCl2 +  2H2O     \n  2NaOH  +  2HCl   =  2NaCl +  2H2O  (the reason for all the 2's is to have the same amount of acid in both equations)\n\nThe mass of calcium hydroxide needed to make up a 1 Molar solution is 74g  ( Ca = 40  O = 16 and H = 1)\n\nHowever you wouldn't be able to make a 1 molar solution of calcium hydroxide as it isn't soluble enough!
382458
H2 + Cl2 -> 2HCl\n2Ag + H2S -> Ag2S + H2 \nCH4 + 2O2 -> CO2 + 2H2O\n2HgO -> 2Hg + O2\n3Fe + 4H2O -> Fe3O4 + 4H2
471546
A.  Iodine is being reduced from +5 in HIO3 to 0 in I2; oxygen is being oxidized from -1 in H2O2 to 0 in O2.\n\nB.  There is no oxidation/reduction going on; this is simple metathesis, producing the barium sulfate precipitate.
964608
There's quite a few. Just google solubility chart. Here's one I found.
983710
H2SO4 will dehydrate and remove water.\n\n\n(CH3)2 CH - CH2-CH=CH-(CH3)2
729117
You don't give the rate law, so it's impossible to tell. Suppose [H2O2] = concentration of H2O2 and [I-] = concentration of iodide. If rate = k[H2O2][I-], then the mechanism is one step. This means that both an H2O2 and an I- have to come together at the same time for the reaction to occur. If rate = k[H2O2], then it's a two-step process. This is because something has to happen to H2O2 in a slow, rate-limiting step, followed by the reaction of whatever with I-.
205870
CaCO3(s) + 2HC2H3O2(aq)-> Ca(C2H3O2)2(aq) + H2O(l) + CO2(g)
770691
CoCl2(aq) + FeSO4(aq) = CoSO4 (aq) + FeCl2(aq)
24810
Cu + 2H2SO4 --> 2H2O + SO2 + CuSO4\nDouble the H2SO4 and the H2O.
560067
According to the solubility rules, it is insoluble.\n\nHere are the solubility rules\n1. All common compounds of Group I and ammonium ions are soluble. \n\n2. All nitrates, acetates, and chlorates are soluble. \n\n3. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides are soluble in hot water.) \n\n4. All sulfates are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I). The latter three are slightly soluble. \n\n5. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble. \n\n6.Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.
944088
CS2 (g) +4H2 (g) <----> CH4 (g) +2H2S(g) \n\na) pressure of CS2 increase,    -  NO\nb) pressure of CH4 decrease,   - NO\nc) pressure of H2 decrease,     -  YES\nd) pressure of H2S decrease,   -  NO\ne) all the pressures will decrease  -  NO
832296
A) Ag2O (s) >>> 2 Ag(s) + 1/2 O2 (g)\nB) Nickel (II) Carbonate >>>>>Nickel (II) Oxide + [Carbon Dioxide], NiCO3 -> NiO + CO2\nC) Ammonium Nitrate >>>>> Dinitrogen monoxide + Water,  \nC does not balance as is... but this does:\nNH3NO3 -> N2O +  1.5 H2O + 0.5 O2\n\n48) A) 2 HCl (aq) + Ca (OH)2 (aq) >>>> 2 H2O + CaCl2 (aq)\nB) 3 Ag2 SO4 (aq) + 2 AlCl3 (aq) >>>> 6 AgCl (s) + Al2(SO4)3 (aq) (silver chloride is a precipitate)\nC) H2C2O4 (aq) + 2 KOH (aq)>>>> 2 H2O + K2C2O4 (aq)\nD) CdBr2 (aq) + Na2S (Aq)>>> CdS(s) + 2 NaBr (aq) (Cadium sulfide is a precipitate)\n50 Write a Balanced equation for the complete combustion of each compound:\nA) Butene (C4H8): C4H8 + 6 O2 -> 4 CO2 + 4 H2O\nB) Octane (C8H18): C8H18 + 12.5 O2 -> 8 CO2 + 9 H2O\nC) glycerol (C3H8O3): C3H8O3 + 3.5 O2 -> 3 CO2 + 4 H2O\nD) Acetone (C3H6O): C3H6O + 4 O2 -> 3 CO2 + 3 H2O\n52: Complete these:\nA) Al (s) + H2SO4 (aq)>>>> AlSO4(aq) + H2(g)\nB) 2 HCl (aq) + Ba (OH)2 (aq)>>>> BaCl2 (aq) + 2 H2O\nC) Au (s) + 3 HCl (aq) >>>>> AuCl3(aq) + 1.5 H2 (g)\n54) EACH IS BALANCED BUT "INCORRECT", so correct these:\nA) Cl-2 + NaI(aq) >>> NaCl2(aq) + I-\nB) NH3(aq) >>> N- + H+3\nC) Na (s) + O2(g) >>NaO2(s)\nD) 2Mg (s) + H2SO4(aq) >>Mg2SO4(aq) + H2(g)\nE) MgCl2(aq) + Ca(OH)2(s) >>> Mg(OH)2(s) + CaCl2(aq)\nF) H2 (g) + Cl2 (g) >> H2Cl2 (g)
991807
uh a pH meter will help with the hydrogen iodide because it's a strong acid.  As for the I2 I have no idea...
108866
the solubility of copper (II) nitrate is 138 g/100 ml of water at 0oC.
5530
Arsenic is the metal, but at temperatures much lower than its melting point (not boiling point).  It sublimes at 614 degrees C and melts under pressure at 817 degrees C.\n\nAlthough Iodine has a metallic luster, it is not a metal.  It sublimes (evaporates) near its \nMelting Point of 114 degrees C.\n\nSee the reference below:
402204
H2SO4 - HCl - H3PO4 - HSO4(1-) - H2PO4(1-) - HPO4(2-)\n\nHCl is quite strong, but suffers the disadvantage at atmospheric pressure that it is volatile and will dissolve in water only up to 37%. It can be driven out of watery solutions by addition of less volatile but not necessarily stronger acids.\n\nH2CO3 would rank fairly high in this list too if you could prevent the CO2 from evaporating.\n\nWhen ranking H2SO4 and H3PO4 you'll have to state how far you want the protolysis to go. Taking the average of H2SO4 and HSO4(1-) makes it weaker than HCl, and worse so for H3PO4.