Calorimetery practical 7: Q= Calculate the enthalpy of neutralization for ( in units of kJ/mol H2O formed ) for both HCl and HAc. Use all parts : a, b and c. [Must use the normal equation and equation: (Specific heat capacity of water x mass of water x change in temp of water ) / (mass of metal x change in temp of water )] Part A Mass of metal (g) - 10.254 Temperature of boiling water bath (°C) 100.4 Mass of calorimeter (g) 4.044 Mass of calorimeter and water (g) 20.519 Time-zero from graph (s) 45.0 Initial temperature of water from graph(°C) 22.3 Final temp = 29.2 Equation of extrapolation curve from graph- y = –0.0047291x + 29.2 Part B Molarity of NaOH (M) 1 Molarity of HCl (M) 1.1 Mass of calorimeter (g) 3.403 Volume of HCl (mL) 50.0 Volume of NaOH (mL) 50.0 Time-zero from graph (°C) 35.5 Initial temperature of mixture from graph(°C) 22.2 Final temperature 29.3 Equation of extrapolation curve from graph y = –0.0017787x + 29.3 Mass of calorimeter and mixture (g) 105.322 Part C Molarity of NaOH (M) 1 Molarity of HAc (M) 1.1 Mass of calorimeter (g) 3.408 Volume of HAc (mL) 50.0 Volume of NaOH (mL) 50.0 Time-zero from graph (°C) 31.5 Initial temperature of mixture from graph(°C) 22.3 Final temperature (TMAX)- 29.1 Equation of extrapolation curve from graph y = –0.0011721x + 26.809 103.775 Mass of calorimeter and mixture (g) 105.116
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Calorimetery practical 7:
Q= Calculate the enthalpy of neutralization for ( in units of kJ/mol H2O formed ) for both HCl and HAc. Use all parts : a, b and c.
[Must use the normal equation and equation:
(Specific heat capacity of water x mass of water x change in temp of water ) / (mass of metal x change in temp of water )]
Part A
Mass of metal (g) - 10.254
Temperature of boiling water bath (°C) 100.4
Mass of calorimeter (g) 4.044
Mass of calorimeter and water (g) 20.519
Time-zero from graph (s) 45.0
Initial temperature of water from graph(°C) 22.3
Final temp = 29.2
Equation of extrapolation curve from graph- y = –0.0047291x + 29.2
Part B
Molarity of NaOH (M) 1
Molarity of HCl (M) 1.1
Mass of calorimeter (g) 3.403
Volume of HCl (mL) 50.0
Volume of NaOH (mL) 50.0
Time-zero from graph (°C) 35.5
Initial temperature of mixture from graph(°C) 22.2
Final temperature 29.3
Equation of extrapolation curve from graph y = –0.0017787x + 29.3
Mass of calorimeter and mixture (g) 105.322
Part C
Molarity of NaOH (M) 1
Molarity of HAc (M) 1.1
Mass of calorimeter (g) 3.408
Volume of HAc (mL) 50.0
Volume of NaOH (mL) 50.0
Time-zero from graph (°C) 31.5
Initial temperature of mixture from graph(°C) 22.3
Final temperature (TMAX)- 29.1
Equation of extrapolation curve from graph y = –0.0011721x + 26.809 103.775
Mass of calorimeter and mixture (g) 105.116
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