Lauren

The specific heat of water is at 4.184J/g * degree C. How much heat is evolved, or absorbed, when the temperature of 9.00 mol of liquid water cools from 38 degrees C to 28 degrees C?

How do I start this problem

  1. 👍
  2. 👎
  3. 👁
  1. q = mass x specific heat x delta T.
    You will need to change the mols of water to grams.

    1. 👍
    2. 👎
  2. wouldnt it be 4.184J/g * degrees C

    so 4.184 J/ 162 g H2O * 10 degrees C = ?

    1. 👍
    2. 👎
  3. mols = grams x molar mass
    9.00 mols H2O x (18.015 g/mol) = ?? g H2O
    q = g H2O x 4.184 J/g*C x delta T
    and delta T = (Tfinal - Tinitial) = (38-28) = -10.
    The answer will be a negative number which means that heat is evolved (and not absorbed).

    1. 👍
    2. 👎
  4. -6783.72 J

    1. 👍
    2. 👎
  5. ok. Actually, if we round the numbers, the last 2 should be a 3. However, if you are concerned about the number of significant figures, the 9.00 limits them to three; therefore, the -6383.73 J would be written as -6.38 x 10^3 Joules.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    1) What Physical properties, other than specific heat, could you use to help identify unknown metals? 2) Why is water an excellent material to use in a calorimeter? Density, color, resistivity (or conductitivy), melting point,

  2. Biology

    What's high specific heat is mainly a consequence of the: A) high specific heat of oxygen and hydrogen atoms B) inability of water to dissipate heat into dry air D) absorption and release of heat when hydrogen bonds break and form

  3. chemistry

    1. Given that 50 grams of ice is heated at -20.0 °C to steam at 135.0 °C. i. Show the graph of the changes from ice to steam ii. Calculate the energy needed to change the ice to steam Please use these values: Heat of fusion =

  4. Chemistry - Heat of Fusion of Ice

    Conclusion question(s) from a lab we did to find the heat of fusion of ice: Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the

  1. chemistry

    An electric range burner weighing 614 grams is turned off after reaching a temperature of 499.0oC, and is allowed to cool down to 22.2oC. Calculate the specific heat of the burner if all the heat evolved from the burner is used to

  2. Chemistry

    How much energy (heat) is required to convert 248 g of water from 0oC to 154oC? Assume that the water begins as a liquid, that the specific heat of water is 4.184 J/g.oC over the entire liquid range, that the specific heat of

  3. Chemistry

    A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C) q =

  4. Chemistry

    The specific heat of water is 4.184J/gc and that of aluminum is 0.897J/gc which substance will show a larger increase in temperature upon the addition of 100J of heat to 100g the aluminum or the water

  1. Science

    Find out the amount of heat required to convert 1 gm of ice at -30 ⁰C to 1 gm of steam at 120 ⁰C. Given the specific heat of ice is 2090 J/kg/⁰C, specific heat of water 4180 J/kg/⁰C, specific heat of steam is 2010

  2. physics

    calculate the heat energy needed to convert 2kg of ice at -12 degree celcius to steam at 100 degree celcius. specific heat capacity for ice=2100j/kg K specific latent heat of ice=340000 J/kg specific latent heat for steam

  3. Chemistry

    Calculate the heat released when 64.5g of steam at 119 C is converted to water at 36 C. Assume the specific heat is 4.184 J/g*C for water, the specific heat of steam is 1.99J/g*C, and the heat of vaporization is 40.79 kJ/mol for

  4. Chemistry

    A sample of silver with a mass of 63.3g is heated to a temperature of 384.4 K and placed in a container water at 290.0K The final temperature of the silver and water is 292.4K assuming no heat loss, what mass of water was in the

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