in  gram and mole , how  many sig figs  do i  star and  end  up  with?
494029
Usually you try and keep as many after the decimal as you can, but sometimes it's only practical to keep about 2 or 3 decimal places. And the number of sig figs you end up with, depends on how many you start with. There's all these rules for adding and multiplying, I could never keep them straight. But generally if you keep the same number of sig figs in your answer as you have at the start, that's ok. Like, 12.01 + 15.999 would be 28.009, but you'd round it off to 28.01, the smallest number of sig figs you were given. That's generally the accepted way. I don't know if that made any sense, but that's the best I can do.
650140
You need to start your values at "0", i.e. for your source data, you need to add 0 as the first entry for both Minutes and Grams (I know nothing about Chemistry but I'm trying to make sense..). That way, when you use the Chart Wizard, the starting point will be 0,0 on your chart. \n\nI think this answers your question, however if my answer sounds as vague to you as it does to me, I've uploaded an image for you to have a look at. Go to: http://i4.tinypic.com/10e0w00.png\n\nGood luck and I hope that helps.
782235
Avagardro's Number = one mole, and all of the masses on the periodic table are in grams/mole.One mole of P equals 30.97g, so d. (c is the only other logical answer, but O2 has a molar mass of 32g/mole beacuse 1 oxygen has a molar mass of 16)\n\nGet used to moles, you'll see them all throughout chemistry.
986618
The equation is already balanced. Count the Ag's on each side = 1. Count the Na's on each side = 1. Count the Cl's on each side = 1. Count the NO3's on each side = 1. One can count the N's on each side = 1, or the O's on each side = 3.\n\nBut one could also consider the question another way:\nAg+ + NO3- + Na+ + Cl- ===> AgCl + Na+ + NO3-
1119792
ger-arg - 1:2\nbra-fra - 1:2\neng-por - 3:1\nita-ukr - 4:0\nI know these are right because i have been to the future...might as well gimme 10 pts right now
860730
Multiply moles by the molecular weight (grams per mol) to get mass (grams).
781614
Na2SO4 (aq) + Ba(NO3)2 (aq) --> 2 NaNO3 (aq) + BaSO4 (s)\n\nThe moles of Barium = 5.00 L * 0.15 mol/L = 0.75 moles\n\nThis is also the moles of sulfate needed:\n\n0.75 mol / 0.36 mol/L = 2.08 L of Na2SO4
810256
With percent, always assume a 100g sample.\n\n21.96% S = 21.96gS\n78.04% F = 78.04gF\n\nConvert grams to moles using molar mass\n\n21.96gS * 1molS/32.06gS = .685 mol S\n78.04gF * 1molF/19.00gF = 4.12 mol F\n\nTake the smallest answer and divide the other by that.  In this case, we'll use .685 mol S.\n\n.685 mol S/.685 = 1 moles S\n4.12 mol F/.685 = 6.01 moles F\n\nNow, just write it out!\nYour empirical formula would be SF6.
808829
g = gram\nkg = kilogram (1,000g) \nmg = milligram (1/1,000g) \nmcg or µg = microgram (1/1,000,000g)
829175
AB + CD ---> AD + CB\nlogic doesn't work here as Si doesn't react/bond with Ca or Phosphorus.and Ca(PO) should be Ca3(PO4)2\nand SiO should be in the form of SiO2. \nso unless you want hypothetical compounds SiO2 won't form with either of the two other reactants.\nbased on the forumlae from an SI data book, the above reaction would not balance.\ngood luck solving this one. :-)
895568
a mole is 6.022×10^23 particles.\n(1.45 * (10^24)) / (6.02200 * (10^23)) = 2.41 moles\n\nN = 14 atomic mass\nO = 16\n\n(14 * 2) + (16 * 5) = 108 g/mole\n(2.41 mole) * 108 (g / mole) = 260.28 grams
967510
Type III Galglioside is a mixture: 20% sialic acid, then equimolar amounts of GM1 and GD1a gangliosides.\n\nA common sialic acid is N-acetylneuraminic acid, with a molecular weight of 310 Da\nGM1 is 49 000 Da\nGD1a is 63 000 Da\n\n1/2 mol each of GD1a and GM1 would weigh 112000 g, meaning it would have a corresponding mass of 28000 g of sialic acid, which is 28000 g/310 g/mol = 90.32 mol\n\nThe mole fractions are therefore 90.32/91.32 = 98.9% for the sialic acid, and 0.5/91.32 = 0.5475% for the 2 gangliosides.\n\nThat makes the average molecular weight equal to 0.989*310 Da + 0.005475 (49000 Da + 63000 Da) = 919.79 Da\n\nThe average molecular weight of the gangliosides, not including the acid, is 56 kDa.
589092
ya you would just go density divided by the mass and then you get the volume  make sure you density is grams/ml and then your mass should be ml and then your volume would turn out to be grams. good luck
483508
I will now quote part of a song our chemistry teacher taught us by Michael Offut\n\n"A mole is a unit, or have you heard?\n Containing 6.02 times 10 to the twenty-third" \n\nor 6.02*10^23
690206
Just slide the decimal over for each multiple:\n\ngiga(G)=1,000,000,000\nmega(M)=1,000,000\nkilo(k)=1,000\nhecto(h)=100\ndeca(D)=10\n1=1 (duh!)\ndeci(d)=.1\ncenti(c)=.01\nmilli(m)=.001\nmicro(that "u" looking thing with a tail)=.000001\nnano(n)=.000000001
1138340
First, you need to multiply this number with the volume you are given in mL to obtain the mass because you are given a density measure (mass per volume). Then, divide by 10^6 because ug means microgram, or a millionth of a gram.
1097097
For grams to mole, you find the molar mass of whatever substance you're working with (add the atomic masses together--it's the number with the decimal on the periodic table), and then put the number of grams you have of the substance over the molar mass.  That gives you the number of moles in the substance.\n\nFor moles to molecules, there are exactly 6.022 x 10^23 molecules of a substance per mole.  That's Avogadro's number.  Simply multiply the number of moles times Avogadro's number and you have the number of molecules.\n\nFor moles to ideal gases, there are 22.4 liters of an ideal gas at standard temperature and pressure per mole of gas.  Multiply your number of moles by 22.4 and you'll have how many liters.