Yes, you are right about density and no, I don't get those answers. For that density sentence I punched x instead of / button. density = mass/volume and
volume = mass/density.
50 g ethanol has v = 50/0.789 or about 60 mL (but you need to do it more accurately). Water has volume of 50/1 = 50 mL . Total 50 + 60 = 110 and percent ethanol = (volume ethanol/total volume) x 100 which is approximately 55%.
1/50 = 0.02 but
1/0.789 is not what you wrote.
25.0 mL of ethanol (density = 0.789 g/mL) initially at 7.0 degrees celsius is mixed with 35.0 mL of water (density = 1.0 g/mL) initially at 25.3 degrees celsius in an insulated beaker. Assuming that no heat is lost, what is the
What pressure (atm) is exerted by a column of ethanol 65.0 cm high? The density of ethanol is 0.789 g/cm3 and 9.8m/s2 as your gravitational constant. mass*gis the weight of the column density*h*area*g= weight density*h*g= pressure
bottle of wine contains 13.1% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality. mass percent _______% molality ______mol/kg
Calculate the molarity and mole fraction of a 2.35 m solution of acetone (CH3COCH3) dissolved in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.) Assume that the final volume equals the sum
At room temperature, ethanol's density is 0.789 g/mL while water's density is 0.997 g/mL. When a few milliliters of ethanol are added to water, the two liquids mix. A student is given a unknown liquid at room temperature and