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So two reactions I performed were: A) Adding 50 cm^{3}water to 0.025 moles CuS0_{4}and measuring ΔT.

B) Adding 50 cm^{3}water to 0.025 moles CuS0_{4}.5H_{2}O and measuring ΔT.

Well turns out the calculations were wrong, since I apparently didn't get kJ/mol but rather mol/40 or so since I didn't take 1 mole of each element.

I want to know whether this was right since my calculations don't yield answers close to the real value otherwise.

∆H reaction = (49.736*4.186*-0.228) /0.025moles= -2 kJ/mol

∆H2 = (51.85*4.186*(-0.929)) /0.025moles= -8 kJ/mol

-2kJ and -8kJ are totally wrong! So I was told about the whole multiply the answer by 40 business.

That gives us: -80-(-320)=-240 kJ which is still not close to the real answer of -11.7 kJ(rough).

I used a temperature sensor, a calorimeter too! What went wrong and how can I correct this? Thanks for your patience this was a lengthy post I hope you can help me solve this problem! :)

Cheers!

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# Caculating the enthalpy change of reaction from delta T values(experimentally)

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