chemistry

the enthalpy of fusion of ice is 6.02 kJ/mol. the heat capacity of liquid water is 75.4 J/molC. What is the smallest number of ice cubes at 0 degrees C each containing one mole of water, necessary to cool 500g of liquid water initially at 20.0 degree C to 0.0 degree C

  1. 👍 0
  2. 👎 0
  3. 👁 113
asked by el
  1. (mass ice*heat fusion) + [mass water x specific heat water x (Tfinal-Tinitial)] = 0
    Solve for mass ice then convert to number of cubes. Remember 1 mole water = 18 grams. The way I read the problem, they don't want any fractional ice cubes. If my interpretation is correct you will calculate the number of ice cubes, then round to the next higher whole number.

    1. 👍 0
    2. 👎 0
  2. 2

    1. 👍 0
    2. 👎 0
    posted by kamlesh
  3. egw

    1. 👍 0
    2. 👎 0
    posted by e

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    How much heat is released when 75.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid

    asked by Bob on April 13, 2010
  2. chem

    How much heat (in kJ) is required to warm 10.0 g of ice, initially at -13.0 ∘C, to steam at 109.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C. The heat capacity of liquid water is 4.18

    asked by Gaby on January 24, 2016
  3. chemistry

    Which of the following constants are needed to calculate the change in enthalpy (H) for heating a sample of liquid water at 10C to steam at 150C. I) the heat capacity of water II) the enthalpy of fusion of water III) the heat

    asked by Bob on January 21, 2011
  4. Chemistry

    DrBob222,HELP! Two 20.0-g ice cubes at –10.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

    asked by Jordan on September 11, 2012
  5. CHEM HELP ASAP!!

    Two 20.0-g ice cubes at –10.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity h2o

    asked by Jordan on September 11, 2012
  6. Chemisty 132

    How much energy (in kilojoules) is needed to heat 5.55g of ice from -13.5 ∘ C to 26.5 ∘ C. The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice and 75.3 J/(K⋅mol) for liquid

    asked by Kayla on September 7, 2014
  7. Chemisty 132

    How much energy (in kilojoules) is needed to heat 5.55g of ice from -13.5 ∘ C to 26.5 ∘ C. The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice and 75.3 J/(K⋅mol) for liquid

    asked by Kayla on September 7, 2014
  8. chemistry

    How much energy (in kilojoules) is needed to heat 4.00g of ice from -11.0∘C to 21.5∘C? The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice and 75.3 J/(K⋅mol) for liquid water.

    asked by Sally on December 13, 2014
  9. chemistry

    How much energy (in kilojoules) is needed to heat 5.45g of ice from -12.0 C to 32.0 C? The heat of fusion of water is 6.01kJ/mol, and the molar heat capacity is 36.6 J/(K x mol) for ice and 75.3 J/(k x mol) for liquid water

    asked by emily on December 2, 2010
  10. Young Harris College

    How much energy is needed to heat 8.50 g of ice from -30.0 C to 70.0 C? The heat of fusion of water is 6.01 kJ/mol, and the molar heat capacity is 36.6 J/(mol.K) for ice and 75.3 J/(mol.K) for liquid water. I got 19.24kJ but it

    asked by Jhon on September 7, 2014

More Similar Questions