Write out the net ionic equations for all three reactions referring to the initial reactions shown in the ‘Background’ section of this template. Be sure to use proper notation when writing your equations as you will include these in the final draft of your report.
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.
Trying to see if I'm on the right track with this lab:
Write out the net ionic equations for all three reactions referring to the initial reactions shown in the ‘Background’ section of this template. Be sure to use proper notation when writing your equations as you will include these in the final draft of your report.
|
Thermochemical Data |
||||||
|
|
Tinitial (°C) |
Tfinal (°C) |
ΔT (°C) |
moles NaOH |
qreaction (kJ) |
ΔHrxn |
|
Reaction 1 |
25.0
|
30.3
|
+5.3
|
0.025 |
-1.11 |
-44.4 |
|
Reaction 2 |
25.0
|
37.0
|
+12.0
|
0.025 |
-2.51 |
-100.4 |
|
Reaction 3 |
25.0
|
31.7
|
+6.7
|
0.025 |
-1.40 |
-56 |
Reaction 1: NaOH(s) → Na+(aq) + OH-(aq) + x1 kJ
1g /39.977g/mol = 0.025 moles
Moles NaOH = 0.025
qsolution = (4.184 J/g °C) (1.0g x 50.0g) (30.3°C -25.0°C)
= 1108.76 J/ 1000
qreaction (kJ) = -1.11 kJ
ΔH = -1.11 kJ/ 0.025 moles
ΔHrxn = -44.4 kJ/mol
Reaction 2: NaOH(s) + HCl(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x2 kJ
1g /39.977g/mol = 0.025 moles
Moles NaOH = 0.025
qsolution = (4.184 J/g °C) (25.0g + 25.0g) (37.0°C -25.0°C)
= 2510.40 J/ 1000
qreaction (kJ) = -2.51 kJ
ΔH = -2.51 kJ/ 0.025 moles
ΔHrxn = -104.4 kJ/mol
Reaction 3: NaOH(s) + HCl(aq) → H2O(l) + Na+(aq) + Cl-(aq) + x3 kJ
1g /39.977g/mol = 0.025 moles
Moles NaOH = 0.025
qsolution = (4.184 J/g °C) (25.0g + 25.0g) (31.7°C -25.0°C)
= 1401.64 J/ 1000
qreaction (kJ) = -2.51 kJ
ΔH = -1.40 kJ/ 0.025 moles
ΔHrxn = -56 kJ/mol
Net Ionic Equations
Reaction 1: NaOH(s) → Na+(aq) + OH-(aq) + -44.4 kJ
Reaction 2: NaOH(s) + HCl(aq) → H2O(l) + Na+(aq) + Cl-(aq) + -104.4 kJ
Reaction 3: NaOH(s) + HCl(aq) → H2O(l) + Na+(aq) + Cl-(aq) + -56 kJ
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
