Measuring Enthalpy (please help I can't understand this at all!)
Q.1 - Using the reaction below, and the enthalpy of formation values, determine the theoretical enthalpy for the reaction from the equation ∆H = ∑HfProducts - ∑HfReactamts
NaHCO3(s) + HC2H3O2(aq) = Na+(aq) + C2H3O2-(aq) + H2O(l) + CO2(g)
(baking soda) (acetic acid)
Hf values in kJ/mol
-HC2H3O2(aq) -486
-NaHCO3(s) -950.8
-Na+(aq) -240.1
-C2H3O2-(aq) -486
-H2O(l) -393.5
-CO2(g) -285.8
Q.2 - Compare the value (+,-) in your lab (photo attached) with the value determined in Q.1. Does the reaction correctly match the definition of exothermic or endothermic? How does the temperature change in the water correlate to the change in the reaction?
Q.3 Compare the number in your lab vs Q.1. What was the size of the error in this experiment?
%error = [tex]\frac{Hf value(Q.1)-experimantal value} {Hf value(Q.1)}[/tex]
Q.4 What are some errors in your setup that could have caused this error? What pieces of equipment would result in a better final heat measurement? Be specific.
