Final Temperature in Calorimeter Thermodynamics Chemistry Questions

Part 1

What is the ΔHorxn of the reaction?

NaOH(aq) + HCl(aq) → H2O(l) + NaCl(aq)

total 150 ml (100 ml HCI and 50 ml NaOH

change in temp 4.11 C

Heat capacity of solution = 4.184 J/goC

Density of solution = 1g/mL

Heat capacity of calorimeter = 32 J/goC

ΔHorxn = ___?_____ kJ/mol

Part 2

NaOH(s) + HCl(aq) → H2O(l) + NaCl(aq)

initial temp 25.00 C

Final temperature 30.70 C. in calorimeter

Heat capacity of solution = 4.184 J/goC

The density of the solution (after NaOH and HCl are mixed) = 1 g/mL

ΔHorxn = ___?_____ kJ/mol HCI =100ml. NaOH 1.0089 g

Part 3

Apply Hess’ Law

Apply Hess’ Law to the experimental result of Question #1 and Question #2 to determine the ΔHrxn of the reaction:

NaOH(s) → NaOH(aq)

ΔHorxn 3= ____?____ kJ/mol

Part 4

NaOH(s) → NaOH(aq)

HCI 100ml

NaoH 1.0359 g

initial temp 25 C

final temp 27.50 C

ΔHorxn = _____?___ kJ/mol