C2H6O = 46.08 g
508 g * (1 mol C2H6O/46.08 g C2H6O) = 11.024 mol C2H6O
There are about 11 moles in 508 grams of ethanol.
9.675 g Since oxygen has an average atomic weight of 15.999 g/mol that would make it 0.21 moles of oxygen. Ethanol has one atom of oxygen per molecule so that means 0.21 moles of ethanol. Since ethanol has a molecular weight of 46.07 g/mole, 0.21 moles of ethanol would have a mass of 9.675 g.
The formula for ethanol is CH3CH2OH So for each mole of ethanol burnt it produces 2 moles of carbon dioxide 1 Mole of ethanol is 46 g 2 moles of carbon dioxide is (2 x 44 g) 88 g So each gram of ethanol produces 1.9 grams of carbon dioxide on combustion
The density of ethanol is 0.789 g/mL. So 19.6 mL of ethanol weighs 0.789 g/mL * 19.6 mL = 15.464 g. The molar mass of ethanol is 2*12.011 + 6*1.008 + 15.999 = 46.069 g/mol. So, in 15.464 grams, there are 15.464 g / 46.069 g/mol = 0.33567 moles In one mole, there are 6.022*1023 molecules, so we have: 0.33567 moles * 6.022*1023 molecules/mole= 2.0214*1023 molecules. Using correct significant digits, that gives: 2.02*1023 molecules (or particles).
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
4.005
9.675 g Since oxygen has an average atomic weight of 15.999 g/mol that would make it 0.21 moles of oxygen. Ethanol has one atom of oxygen per molecule so that means 0.21 moles of ethanol. Since ethanol has a molecular weight of 46.07 g/mole, 0.21 moles of ethanol would have a mass of 9.675 g.
Unless I've completely forgotten my chemistry, mole fraction is the fraction of moles of a particular solute of the entire number of moles in the solution. So for this question: formula weight of ethanol = 46.07 g/mol formula weight of water = 18.015 g/mol moles of ethanol = 47.5g / 46.07 g/mol = 1.0310 mol moles of water = 850g / 18.015 g/mol = 47.182 mol total number of moles in the solution = 1.0310 + 47.182 = 48.213 mol therefore, the mole fraction of ethanol is 1.0310 mol / 48.213 mol = 0.0214 hope this helps.
The formula for ethanol is CH3CH2OH So for each mole of ethanol burnt it produces 2 moles of carbon dioxide 1 Mole of ethanol is 46 g 2 moles of carbon dioxide is (2 x 44 g) 88 g So each gram of ethanol produces 1.9 grams of carbon dioxide on combustion
32 g ethanol is equivalent to 0,695 moles.
5.0M Molarity is moles of solute/liters of solution. The molar mass of ethanol is 46.07 g/mol, so 115g of ethanol is 2.5 moles of ethanol. 500cc is the same as 0.5L. So 2.5 mol/0.5L = 5.0M
The number of moles is mass in g/molar mass in g.
The formula is: number of moles = g Be/9,012.
The number of moles 9,92.10e-5.
0.0027 moles.
Number of moles is determined by dividing molar mass into the number of grams. SO2 has a molar mass of 64.066 g. To find the number of moles in 250.0 g of SO2, divide 250.0 g by 64.066 g. This gives you just over 3.9 moles.
22.99 g of C28H44O is equal to 0,058 moles.
510 g Al2S3 is equal to 3,396 moles.