At a certain elevation, the boiling point of water is 98.5°C. How much energy is needed to heat 35.0 mL of water to the boiling point at this elevation if the water initially was at 23.4°C?
(Cp=75.38J/(mol*C), d= 1.00g/mL)

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  1. q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
    Tfinal = 98.5 C
    Tinitial = 23.4 C

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  2. 11.0kJ

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