Hess\' Law Lab Questions PDF

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1) My molar enthalpy change values for reactions 2 and 4 were very similar. For reaction 2, the molar enthalpy change was -24.7 kJ/mol and for reaction 4, the molar enthalpy change was -25.7. This is because their net ionic equations are similar too. For reaction 2, the net ionic equation only involves a hydrogen ion and a hydroxide ion to make liquid water. For reaction 4, the net ionic equation involves a hydrogen ion with sodium hydroxide to make a sodium ion and liquid water. Yes, my experimental values follow this pattern. 2) The results of reactions 1, 2, and 3 should have similar molar enthalpy change values. This is because their reactions include sodium hydroxide with water and then sodium hydroxide with hydrochloric acid to make water. Hess’ Law states that only the result matters, not how that result was achieved. These reactions are a good example of Hess’s Law because they all start with sodium hydroxide and have very close values for molar enthalpy change. 4) For all of my trials, the error is large partly because I may have calculated my values incorrectly. 5) No, the theoretical molar enthalpy change values for the trails don’t agree with what I said for question 1. The theoretical values are very different from each other. They don’t agree with the Hess’ Law as I described for my answer in question 2 either. 6) -0.351 kJ/mol + (-24.7 kJ/mol) = -25.051 Reaction 3 molar enthalpy chnage = -24.2 kJ/mol...