I have to calculate the ΔV= final volume-initial volume
For the first trial the final volume was .005mL the initial volume was .03mL, which equaled to
-.025mL. The volume was negative because it was exothermic reaction. For the second trial the final volume was 0.015 and the initial volume was 0.03, which equaled to -.015mL.
Now I have to convert ΔV to ΔH273 values. TheΔH273 is the molar enthalpy change for the reaction of the magnesium metal. How do I compute the mean value of ΔH273?
ΔH=ΔE +nRT
Also calculate the ΔE273 from the mean value of ΔH273?
The equation for the reaction that took place was: Mg(s) +2H+(aq)→Mg+2(aq) +H2 (aq)