A one liter aqueous solution contains 18g C6H12)6 and 3.2g CH3OH. What is the mole fraction of C6H12O6


the destroyer says that 1L= 1000g H2O and we need to convert this into mols too......is that something we're just supp to know that 1L=1000g H2O bc it wasnt given in the question....and do we use convert 1000g of H20 to mol everytime in a mole fraction question if its asked in an aqueous solution if this is the case?

since it's referring to mole fraction, you have to consider all the stuff in the solution which includes water. That's why you have to also take into account the moles of water along with the other solutes. As for knowing 1L = 1000g, that only works for water I believe. I suppose it can't hurt to know it but I doubt they would ask you to know that on the real Dat.

that's also only because the density of water is 1g/mL.