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Enthalpy Change Calculation

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
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white-rose
Deta h is -q/n

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