chemistry

29.8 ml of ethanol (density = 0.789 g/ ml) initially at 9.9 degree celsius is mixed with 33.8 mL of water (density = 1.0 g/mL) initially at 27.8 degree celcius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of mixture?
How do I start this problem?

  1. 👍 0
  2. 👎 0
  3. 👁 232
asked by June
  1. heat gained by ethanol + heat lost by water = 0
    heat gained by ethanol = mass x specific heat x (Tfinal-Tinitial). Use density to convert mL to mass.

    heat lost by water = mass x specific heat x (Tfinal-Tinitial). Use density to convert mL to mass.
    Tfinal is the only unknown.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    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

    asked by Elle on February 9, 2012
  2. chemistry

    If 51.6 mL of ethanol (density = 0.789 g/mL) initially at 6.4°C is mixed with 48.9 mL of water (density = 1.0 g/mL) initially at 29.1°C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of

    asked by MK on October 15, 2013
  3. Chemistry I

    25.0 mL of ethanol (density = 0.789 g/mL) initially at 4.2°C is mixed with 35.7 mL of water (density = 1.0 g/mL) initially at 25.3°C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the

    asked by Robbie on September 15, 2010
  4. chemistry

    25.0 mL of ethanol (density = 0.789 g/mL) initially at 5.5°C is mixed with 32.3 mL of water (density = 1.0 g/mL) initially at 25.3°C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the

    asked by Anonymous on September 19, 2014
  5. chemistry

    25.6mL of ethanol (density =0.789 g/mL) initially at 5.4∘C is mixed with 30.4mL of water (density = 1.0 g/mL) initially at 20.4∘C in an insulated beaker.Assuming that no heat is lost, what is the final temperature of the

    asked by Lisa on September 12, 2014
  1. Chemistry

    20.7mL of ethanol (density=0.789g/mL) initially at 8.2 degrees Celsius is mixed with 37.1 mL of water (density=1.0g/mL) initially at 25.7 degrees Celsius in an insulated beaker. Assuming that no heat is lost, what is the final

    asked by Katie on February 7, 2012
  2. chemistry

    25.6 {\rm mL} of ethanol (density =0.789 {\rm g}/{\rm mL}) initially at 8.0^\circ {\rm C} is mixed with 39.5 {\rm mL} of water (density = 1.0 {\rm g}/{\rm mL}) initially at 23.1^\circ {\rm C} in an insulated beaker. Assuming that

    asked by MD on February 22, 2012
  3. Chemistry

    20.0 mL of ethanol initially at 7.2 degrees Celsius is mixed with 31.7 mL of water initially at 28.9 degrees Celsius in an insulated beaker. Assuming no heat is lost, what is the final temp? I did not include the density, but I

    asked by Jennifer on January 8, 2016
  4. math

    what is the mass of 1.00 L of ethanol? Ethanol has a density of 0.798 g/ml. (hint: one liter is 10^3 mL.) A. 0.789 g B. 789 g C. 789 L I think C

    asked by shana on November 7, 2012
  5. chemistry

    Calculate the final temperature of 34mL of ethanol initially at 13∘C upon absorption of 938J of heat. (density of ethanol =0.789 g/mL)

    asked by Dylan on September 10, 2014

More Similar Questions