A bottle of win contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is .79 g/mL. Calculate the concentration of ethanol in wine as mass percent and molality.

I calculated molality as 2.4 m/kg, but I'm stumped on the mass percent [although I'm hitting the right area.] Is the solvent water?

I calculated the molality as 2.45 mols/kg solvent so I assume you are doing that part correctly.

For percent by mass.
12.5 v/v percent is
12.5 mL EtOH in (12.5 mL EtOH + 87.5 mL H2O).
12.5 mL with density of 0.79 g/mL = 9.875 g.
mass %= [mass EtOH/(mass EtOH + mass H2O)]x 100 =
[9.875g/(9.875 g + 87.5 g)]x100 = 10.14 w/w percent.
Check my thinking. Check my arithmetic.

  1. 👍
  2. 👎
  3. 👁
  1. It comes out to be 10.2. Check your math and do it over again. Your very close to the answer

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. AP Chemistry

    A bottle of wine contains 12.5% 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.

  2. Chemistry

    A solution is prepared by mixing 1.00g ethanol (C2H5OH) with 100.0g water to give a final volume of 101.mL. Calculate the molarity, mass percent and mole fraction of ethanol in the solution.

  3. Chemistry

    The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.

  4. Chemistry

    What is the mass/ vol% ethanol in an ethanol water solution with density of 0.875g/ml and containing 65% ethanol by volume? The density of pure ethanol is 0.789g/ml? My calculation 0.875g/ml x 1000ml x 0.65/ 46.06 = 12.34m

  1. chemistry

    Calculate enthalpy change of reaction for the combustion of gaseous ethanol. C2H5OH + 3O2 >> CO2 + 3H2O. Using standard molar enthalpies of formation. C2H5OH -235.3 ( it's negative sign) CO2 -393.5 H2O -241.8 (1) Calculate the

  2. Chemistry

    What mass of water must be used to dissolve 20.0 grams of ethanol, C2H5OH, to prepare a 0.0500 molal solution of ethanol?

  3. chemistry

    The complete combustion of ethanol, C2H5OH (FW = 46.0 g/mol), proceeds as follows: C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔH = −555 kJ What is the enthalpy change for combustion of 15.0 g of ethanol

  4. Chemistry

    Wine is approximately 12% ethanol (CH3CH2OH) by volume. Ethanol has a molar mass of 46.06 g/mol and a density 0.789 g/mL. How many moles of ethanol are present in a 750-mL bottle of wine?

  1. chemistry

    A solution of ethanol, C2H5OH, is prepared by dissolving 25.0 mL of ethanol in enough water to give a total volume of 250.0 mL. What is the percent-by-volume concentration of ethanol?

  2. Chemistry

    A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00°C to 33.73°C. If the heat capacity of the calorimeter and contents was 9.63

  3. chemistry

    Please help =) 59. Ethanol, C2H5OH, is responsible for the effects of intoxication felt after drinking alcoholic beverages. When ethanol burns in oxygen, carbon dioxide and water produced. (a) Write a balanced equation for the

  4. chemistry

    Ethanol, C2H5OH, is being promoted as a clean fuel and is used as an additive in many gasoline mixtures. Calculate the ΔH°rxn for the combustion of ethanol. ΔH°f [C2H5OH(l)] = -277.7 kJ/mol; ΔH°f [CO2(g)] = -393.5 kJ/mol;

You can view more similar questions or ask a new question.