You need the balanced symbol equation for the reaction. The numbers in front of the formulae show the mole ratios. For example, in the thermal decomposition of calcium carbonate:
CaCO3 --> CaO + CO2
The equation is balanced.
The mole ratio between CaCO3 and CO2 is 1:1 because there is 1 mole of CaCO3 for every mole of CO2
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∙ 14y agoWiki User
∙ 11y agoMole percent is the mole fraction (X) for a component of a mixture times 100.
If you have a solution of 5.0g NaCl and 25.0g H2O, you can find the mole fraction and mole percent for each. The sum of all percents of all of the components of a mixture equals 100.
Determine the moles (n) of NaCl and H2O.
5.0g NaCl x 1mol NaCl/58.44g NaCl = 0.086mol NaCl
25.0g H2O x 1mol H2O/18.016g H2O = 1.39mol H2O
Determine mole fractions (X) of NaCl and H2O.
The sum of all mole fractions in a solution = 1.
XNaCl = nNaCl/(nNaCl + nH2O) = 0.086mol NaCl/(0.086mol NaCl + 1.39mol H2O) = 0.58mol NaCl
XH2O = 1 - 0.58mol = 0.42mol H2O
Determine the mole percent of NaCl and H2O.
Mole percent of NaCl = XNaCl x 100 = 0.58 x 100 = 58%
Mole percent of H2O = XH2O x 100 = 0.42 x 100 = 42%
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∙ 12y agoMole fraction and mole percent are essentially describing the same quantity, only mole percent uses the conversion of a number to a percentage. That's all the difference there is. Hence, a mole fraction of 0.134 for a component in a mixture is equivalent to 13.4 % in mole percent of that component. Mole percent spans the range from 0 to 100% while mole fraction spans the real values from 0 to 1.
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∙ 13y agomole fraction= moles of component/total numbers of moles of components
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∙ 14y agonumber of moles of solute/solvent divided by number of moles of the solution
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∙ 15y agoMole Fraction formulaMole fraction is the number of moles of a substance divided by the total number of moles in the solution.Mole Fraction =moles of substance ATotal Moles of solution
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∙ 9y agoMole fraction to volume fraction could be converted using the molar mass and the density of the particles involved in the liquid.
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∙ 11y agoMultiply moles times the molar mass of the substance in grams/mole.
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∙ 11y ago(mole of solute/mole of solvent)*100
you convert it to g/mole. Think of Mole as the word "dozen." Whenever you see the word "mole" just cross it out and put in the word "dozen". Do the problem like that, and then change all of your dozens to 6^1023. A dozen is 12. A bakers dozen is 13 and a mole is....whatever...some other big number. It doesnt matter. How do you calculate mass of a liquid in grams/dozen? You usese it's atomic weight which is in grams and then convert.
Henry's law states that, the partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.
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Like a pressure, but with non-ideality Use as a pressure Fugacity = mole fraction of gas * total pressure Mole fraction of CO2 in atmosphere? 383 ppmv
1 mole of every gas has a volume 22.414 dm3 at S.T.P.
For Ideal gases, mole fraction=volume fraction
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
because mole fraction doesnot depend on volume
the mole fraction of oxygen= 37/100 0.37 the mole fraction of Nitrogen= .63 that equals to give 1
Your question doesn't have a single answer. In Chemistry solution strength is usually calculated in moles pe liter of mole per kilogram or as a mole fraction ( moles per mole) but can also be mass per liter, mass per mass, volume per volume, percent by mass, or percent by volume.
you convert it to g/mole. Think of Mole as the word "dozen." Whenever you see the word "mole" just cross it out and put in the word "dozen". Do the problem like that, and then change all of your dozens to 6^1023. A dozen is 12. A bakers dozen is 13 and a mole is....whatever...some other big number. It doesnt matter. How do you calculate mass of a liquid in grams/dozen? You usese it's atomic weight which is in grams and then convert.
as we define mole to be mass of the solute divided by molecular mass of the solute so all the solutes are taken in the solid form not in the liquid like we take 1L in molarity,so solids are generally independent of temp thats why both molality and mole fraction are independent of temperature
The mole fraction and molality of ethanol -C2H5OH in an aqueous solution that is 45.0 percent ethanol by volume and the density of water is 1.00g per mL that of ethanol is 0.789 grams per mL and 70/18. A mole fraction in chemistry is the amount that is divided by the total amount of all constituents.
The mole fraction of Oxygen = 21/100= .21
The mole fraction of HCl is 0.34.
Assuming I've understood what you're trying to ask: first calculate the mass, then convert that to a volume using the density.
Mole is not a unit of volume. Mole deals with numbers like dozen.