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    Calculate the energy in the form of heat (in kJ) required to change 50.0 g ice at –15.0 °C to liquid at 65.0 °C. (Heat of fusion = 333 Jg–1; heat of vaporization = 2256 Jg–1; specific heat capacities: ice = 2.06 Jg–1K–1, liquid water = 4.184 Jg–1K–1)
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    Aliens.
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    We aren't doing your homework for you. This forum is only for help.
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    (Original post by johnny k)
    Calculate the energy in the form of heat (in kJ) required to change 50.0 g ice at –15.0 °C to liquid at 65.0 °C. (Heat of fusion = 333 Jg–1; heat of vaporization = 2256 Jg–1; specific heat capacities: ice = 2.06 Jg–1K–1, liquid water = 4.184 Jg–1K–1)
    Think about the stages involved in heating the ice. You need to work out the energy change needed to heat ice to its melting point, the energy needed to melt it, and the energy needed to then heat that water to 65.0 °C.
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    Also, aliens.
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    I'm not sure if this is correct, so don't quote me on it, but you could use the formula of E=mc deltaT -sorry couldn't find the symbol.

    Because you're trying to work out E and you're given the specific heat capacity (deltaT) also the temperature difference, and also the mass of water (50g)

    hope this helps
 
 
 
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