Anonymous asked in Science & MathematicsChemistry · 1 decade ago

Energy needed to convert 52g ice @ -10C to steam @100C?

Specific heat of ice: 2.09 J/g C deltaH fus = 6.02kJ/mol

Specific heat of water: 4.18 J/g C deltaH vap = 40.7 kJ/mol

Specific heat of steam: 1.84 J/g C

3 Answers

  • 1 decade ago
    Favorite Answer

    You need to break it down. Energy when not in a phase change is Q=mc(deltaT) whereas energy at a phase change is Q=deltaH(m)

    So from -10C to 0C, no phase change occurs and it is ice:

    Q=52g*2.09 J/g C*(10C)= 1086.8J=1.087kJ

    At 0C, melting occurs, so you use deltaH fusion:

    Make sure your units work out properly:

    Q=6.02kJ/mol(52g)(1mol/18g) = 17.39 kJ

    From 0C to 100C, no phase change occurs when it's liquid:

    Q=52g*4.18 J/g C*(100C)= 21736J=21.736 kJ

    At 100C, phase change occurs as water evaporates:

    Q=40.7kJ/mol*52g*(1mol/18g) = 117.6 kJ

    Add these values of heat up: 1.087 + 17.39+21.736+117.6=157.8 kJ

  • darien
    Lv 4
    4 years ago

    looks there's a Ben & Jerry's ice cream it somewhat is espresso with chunks of chocolate and peanut butter. i may well be incorrect on that. If there is not any longer then i might elect to invent it and patent it too, lol! Sooo, my answer after it is espresso Ice cream!

  • 1 decade ago

    105 j/g DF x 21 mJ/g SQ2 / omega C

    (Specific homework cheating) SQ3 # D at the end of the semester

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