Topic: Sublimation and Fusion

How much heat (in kJ) is required to warm 13.0 g of ice, initially at -14.0 C, to steam at 112.0 °C? The heat capacity of ice is 2.09 J/g⋅°C and that of steam is 2.01 J/g⋅°C.

Any help on how to start this is really appreciated.

  1. 👍
  2. 👎
  3. 👁
  1. Do this in several steps.
    heat to raise T ice at -14 C to zero.
    heat to melt ice at zero.
    heat to raise T from zero to 100 C.
    heat to vaporize water at 100.
    heat to raise steam from 100 to 112 C.
    The total is the sum of each part above.
    Post your work if you get stuck.

    1. 👍
    2. 👎
  2. Step 1: Heat to raise T of ice at -14.0 °C to 0.0 °C

    q_1 = m⋅C_s,ice⋅ΔT
    q_1 = (13.0 g)(2.09 J/g⋅°C)[0.0 °C - (-14.0 °C)]
    q_1 = 380.38 J
    q_1 = 0.38038 kJ

    Step 2: Heat to melt ice at 0.0 °C

    q_2 = n⋅ΔH_fus
    q_2 = [13.0 g⋅(1 mol/18.016 g)⋅(6.02 kJ/mol)
    q_2 = [13.0 g⋅(1 mol/18.016 g)]⋅(6.02 kJ/mol)
    q_2 = 4.343916519 kJ

    Step 3: Heat to raise T of water from 0.0 °C to 100.0 °C

    q_3 = m⋅C_s,liq⋅ΔT
    q_3 = (13.0 g)(4.18 J/g⋅°C)(100.0 °C - 0.0 °C)
    q_3 = 5434 J
    q_3 = 5.434 kJ

    Step 4: Heat to vaporize water at 100.0 °C

    q_4 = n⋅ΔH_vap
    q_4 = [13.0 g⋅(1 mol/18.016 g)⋅(40.7 kJ/mol)
    q_4 = [13.0 g⋅(1 mol/18.016 g)]⋅(40.7 kJ/mol)
    q_4 = 29.36833925 kJ

    Step 5: Heat to raise T of water from 0.0 °C to 100.0 °C

    q_5 = m⋅C_s,steam⋅ΔT
    q_5 = (13.0 g)(2.01 J/g⋅°C)(112.0 °C - 100.0 °C)
    q_5 = 313.56 J
    q_5 = 0.31356 kJ

    Total Heat Required

    q_1 + q_2 + q_3 + q_4 + q_5
    (0.38038 kJ) + (4.343916519 kJ) + (5.434 kJ) + (29.3683392 kJ) + (0.31356 kJ)
    39.84019572 kJ

    I'm fairly certain I used the correct values for the heat capacities and the heat of fusion and heat of vaporization. Is this correct?

    1. 👍
    2. 👎
  3. The procedure looks ok. I didn't look up the Cp values but I know 4.18 is ok for liquid water. I didn't check the math but I note that you need to watch the number of significant figures. I think 3 s.f. are allowable.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Lead has a melting point of 327ºC, its specific heat is J/g•deg, and its molar enthalpy of fusion is 4.80 kJ/mol. How much heat, in kilojoules, will be required to heat a 500.0-g sample of lead from 23.0ºC to its melting point

  2. Chemistry

    How many kilojoules of heat are required to melt a 10.0 g popsicle at 0 degress C? Assume the popsicle has the same molar mass and heat of fusion as water. Could someone tell me what equation to use to solve this or the steps?

  3. physics

    The melting point of a solid is 90.0 d/C. What is the heat required to change 2.5 kg of this solid at 40.0 d/C to a liquid? The specific heat of the solid is 390 J/kg-K and its heat of fusion is 4000 J/kg. I got 2 different

  4. Chemistry

    22.) The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/gC. (1) What quantity of heat is required to melt 25.0 g of ice at

  1. Chemistry

    How much heat is required to warm 122g of water by 23.0°C? Specific heat is 4.184 J/g° C. Please show work:(((

  2. Chemistry

    The specfic heat of iron is 0.11cal/g C. The heat of fusion of iron, the heat required to convert iron from a solid to liquid at its melting point, is 63.7cal/g. Iron melts at 1530 C. How much heat must be added to 2g of iron at

  3. Chemistry

    Calculate the number of joules required to melt 57.4g of benzene at 5.5 degrees celsius? The heat of fusion for benzene is 9.87 KJ/mol and specific heat for liquid benzene is 1.63 J/g*deg)

  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. Math

    A heat exchanger is used to warm apple cider using steam as the heat source. The cider is heated from an initial temperature of 4°C to a final temperature of 65°C. The steam enters the heat exchanger as 50% quality steam and

  2. Chemistry

    Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 25.0°C to gaseous CCl4 at 76.8°C (the normal boiling point for CCl4)? The specific heat of CCl4(l) is its heat of fusion is and its heat of

  3. Physics

    The melting point of a solid is 90.0 degrees C. What is the heat required to change 2.5 of this solid at 40.0 degrees C to a liquid? The specific heat of the solid is 390 J/kg (K) and its heat of fusion is 4000 J/kg. A. 4.9 10^4 J

  4. physics

    calculate the amount of heat energy required to melt a 1kg iron ingot initially at 20 ¡ãC? (heat of fusion for Fe is 33.0 J/g

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