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    Enthalpy Cycle

    Part A: Determine the enthalpy change when 0.025 moles of anhydrous CuSO4(s) is dissolved in 50cm3 of water

    temp went up by 8C

    Enthalpy change = mc?t
    Enthalpy change = 50*4.18*8
    Enthalpy change for 0.025 mols = 1672J or 1.672kJ

    so ?H1 = 1.672*40 = 66.88

    Part B: Determine the enthalpy change when 0.025 moles of CuSO4.5H20 is dissolve in enough water to make 50cm3 of CuSO4 Solution.

    so 47.75cm3 of water is needed

    temp went up 1 degree

    Enthalpy change = 47.75*4.18*1 = 199.595J
    Enthalpy change for 0.025 mols = 0.199595kJ

    so ?H2 = 0.199595*40 = 7.9838

    Is this correct so far? and if it is how do I calculate Delta h

    Deta h is -q/n
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