Ask Question
14 September, 20:07

Calculate the amount of energy in kilojoules needed to change 369 gg of water ice at - -10 ∘C∘C to steam at 125 ∘C∘C. The following constants may be useful: Cm (ice) = 36.57 J / (mol⋅∘C) Cm (ice) = 36.57 J / (mol⋅∘C) Cm (water) = 75.40 J / (mol⋅∘C) Cm (water) = 75.40 J / (mol⋅∘C) Cm (steam) = 36.04 J / (mol⋅∘C) Cm (steam) = 36.04 J / (mol⋅∘C) ΔHfus=+6.01 kJ/molΔHfus=+6.01 kJ/mol ΔHvap=+40.67 kJ/molΔHvap=+40.67 kJ/mol Express your answer with the appropriate units.

+3
Answers (1)
  1. 14 September, 21:01
    0
    We need 1136.4 kJ energy

    Explanation:

    Step 1: Data given

    The mass of water = 369 grams

    the initial temperature = - 10°C

    The finaltemperature = 125 °C

    Cm (ice) = 36.57 J / (mol⋅∘C)

    Cm (water) = 75.40 J / (mol⋅∘C)

    Cm (steam) = 36.04 J / (mol⋅∘C)

    ΔHfus=+6010 J/mol

    ΔHvap=+40670 J/mol

    Step 2: : Calculate the energy needed to heat ice from - 10 °C to 0°C

    Q = n*C*ΔT

    ⇒Q = the energy needed to heat ice to 0°C

    ⇒with n = the moles of ice = 369 grams / 18.02 g/mol = 20.48 moles

    ⇒with C = the specific heat of ice = 36.57 / J/mol°C

    ⇒ ΔT = the change of temperature = 10°C

    Q = 20.48 moles * 36.57 J/mol°C * 10°C

    Q = 7489.5 J = 7.490 kJ

    Step 3: calculate the energy needed to melt ice to water at 0°C

    Q = n * ΔHfus

    Q = 20.48 moles * 6010 J/mol

    Q = 123084.8 J = 123.08 kJ

    Step 4: Calculate energy needed to heat water from 0°C to 100 °C

    Q = n*C*ΔT

    ⇒Q = the energy needed to heat water from 0°C to 100 °C

    ⇒with n = the moles of water = 369 grams / 18.02 g/mol = 20.48 moles

    ⇒with C = the specific heat of water = 75.40 J / (mol⋅∘C)

    ⇒ ΔT = the change of temperature = 100°C

    Q = 20.48 moles * 75.40 J/mol°C * 100°C

    Q = 154419.2 J = 154.419 kJ

    Step 5: Calculate energy needed to vapourize water to steam at 100°C

    Q = 20.48 moles * 40670 J/mol

    Q = 832921.6 J = 832.922 kJ

    Step 6: Calculate the energy to heat steam from 100 °C to 125 °C

    ⇒Q = the energy needed to heat steam from 100 °C to 125 °C

    ⇒with n = the moles of steam = 369 grams / 18.02 g/mol = 20.48 moles

    ⇒with C = the specific heat of steam = 36.04 J / (mol⋅∘C)

    ⇒ ΔT = the change of temperature = 25 °C

    Q = 20.48 moles * 36.04 J/mol*°C * 25°C

    Q = 18452.5 J = 18.453 kJ

    Step 7: Calculate total energy needed

    Q = 7489.5 J + 123084.8 J + 154419.2 J + 832921.6 J + 18452.5 J

    Q = 1136367.6 J

    Q = 1136.4 kJ

    We need 1136.4 kJ energy
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Calculate the amount of energy in kilojoules needed to change 369 gg of water ice at - -10 ∘C∘C to steam at 125 ∘C∘C. The following ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers