identify the percent; a chemical is 42% pure, of 800 grams of the chemical, how much is pure/?
398472
.42 X 800 = (you do the math)
404126
Wt percent:\n\nC atomic weight: 12\nCO3 molecular Wt : 44\n% wt = 12X100/44 = 27.3%
810837
Just remember glucose (C6H12O6). Then using the basics of balancing any chemical equation you can figure out the rest of it.
583365
First of all work out the molar mass of CuSO4*5H2O\n Cu + S + (9 * O) * (10 * H)\n\nSorry I don't have a chemical table next to me\n\nCall this A\n\nSecondary work out the mass of 5 moles of water.\nCall this B\n\n(5 * O) + (10 * H)\n\nthe theoretical % is then B/A * 100 = x%
5197
More information is needed.  What is the concentration is it a percentage or a molarity.\n\nDo you need to find the concentration or just the amount of alchohal?
87793
44.00995 grams per mole
24464
Group 6A contains oxygen, sulfur, selenium and tellurium.\n\na) Any of these form ions with a double negative charge.\n\nb) consequently, the formular can be expected to be Al2X3\n\nc) 18.55% percent Aluminium by mass means that 81.45% of the mass is taken up by X.\n\nThat's 9.275% per Aluminium ion and 27.15% per X ion.\n\nTo determine the atomic mass of X, you take the atomic mass of Aluminium (27 is exact enough for our  purposes), divide it by the mass percentage per Al ion and multiply by the mass percentage per X ion:\n\n27 / 9.275 * 27.15 = 79\n\nA quick look into the periodic table reveals that this is the atomic mass of Selenium.
976426
You can't tell from that.  You didn't say how concentrated the BaCl2 solution was.  To solve this problem, first multiply the molarity (moles per liter) of the solution by the volume of the soution in liters (0.025 in this case).  That gives you the number of moles of BaCl2 you started with.  \n\nThen, calculate the molar mass of BaSO4.  You can find the atomic weights of the elements on your periodic table.  The molar mass is the sum of the atominc masses--the mass of Ba, the mass of S, and four times the mass of O.  Add all that up and you've got the molar mass.  This is what one mole of BaSO4 weighs, or the grams per mole.  \n\nTake the reciprocal of the molar mass (1/molar mass) to get the number of moles per gram, and multiply this by 0.8 grams to get the number of moles recovered.  Then to get an absolute value for the amount of Ba2+ unreacted, just subtract the moles recovered from the starting moles.\n\nTo get the percent unreacted, take the moles unreacted from the last step, divide by the starting moles, and multiply by 100%.
132551
3 and a half grams.  An 8th of an ounce.
847953
If you know the mass ratio of the components of a compound you can determine the empirical formula.  What you have to do is convert the mass ratio into a percentage of the compound.  Then assuming you have a 100 gram sample the percentages would be the grams of each element.\n\nThen divide the grams of each element by each element's atomic mass.  This gives you the moles.\n\nThen divide the moles of each element by the smallest value to get an integer value.  If one or more of the values is not an integer, multiply by the smallest number you can to get whole numbers.  Then the numbers will be the number of atoms of each element in the compound.\n\nYou determine the mass ratio by quantative analysis.
342540
Take the mass of the substance of interest, divide it by the total mass, mulitply by 100.\n\nIf you need to find the percent of an element within a compound, you convert mass of the compound to moles, and then determine the number of moles. \n\nThe number of moles of the compound will be equal to the number of moles of the element multiplied by however many atoms of that element are in the compound.\n\nFor example, if you have 3 moles of NH4OH, then you have 3 moles of N in that compound, and 15 moles of H in the same compound.\n\nOnce you have the number of moles of your element of interest, you convert it back to grams. Then divide that by the total weight of the compound and multiply by 100.\n\nHope I haven't been too confusing.
1186593
Mix with a 0% solution in the relation 33:2\n\nSo use 2 units of your solution (like 2 liters) and 33 units of the 0% solution (like 33 liters).\n\nThat's all.
878037
Suspect this is what you mean...\n\nSuppose you have 0.500 g of a substance you believe is pure...\nyou analyse it and determine that it contains 0.300 g of the substance you are looking for..\nso your sample is (0.300/0.500) x 100% pure  = 60%
69413
56.4% of 220 g/mol is ___ grams of P /mol of oxide 1.\n\n43.6% of 284 g/mol is ___ grams of P /mol of oxide 2.\n\nAnalogous for the oxygen content.\n\nMultiply and round to the next whole number.\n\nOk. Oxygen has the molar mass 16. Seeing the difference between the two oxides is 64, oxide 2 holds 4 oxygen atoms more than oxide 1.\n\nLacking a convenient calculator nearby, I'll guess that 43.6%*220 g/mol yields 96 g/mol, or 6 oxygen atoms per mol of oxide 1. That leaves 124 g/mol phosphorous, with a molar mass of 31 this yields 4 atoms of P. P*4 + O*6, or P4O6, three-valent P.\n\nOxide 2 has 4 oxygen atoms more: P4O10, 5-valent P.
888514
density=__g/ml   that means density equals __grams per millileter
95798
I'm thinking concentration, but your question is worded sort of oddly... Does that fit with what you've been learning????  It's usually percent by mass I think...
118416
MY ANSWER IS:\n\n1 mol/g of LiCl = 35.4g