Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide. Show your work. If you are including a scan of your handwritten work, it must be legible.
Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide. Show your work. If you are including a scan of your handwritten work, it must be legible.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Transcribed Image Text:+
Room Temperature
Reactant
Trial Number
Mass of reactant (from data)
Moles of reactant (calculate)
Initial time (ti) (from graph)
Initial Temperature (Ti)
(from the graph)
Linear Curve fit slope (m)
(from the graph)
Linear Curve fit intercept (b)
(from the graph)
Final Temperature (T)
(calculate from linear fit data)
AT = T₁-Ti
awater
calorimeter
arxa
AHrxn
26.0°C
Mg(s) + ½ O₂ (g) → MgO (s)
Mg
0.2578 g
1
0.0106 mol
33.5 s
24.3°C
37.23 °C
37.06 °C
12.8 °C
5355.52 J
(5.36 kJ)
128 J
Mg
-5483.52 J
2
0.2551 g
0.0105 mol
41.05 s
29.055 °C
41.72 °C
41.46 °C
12.41 °C
5192.344 J
(5.192 kJ)
-0.005191 °C/s -0.006452 °C/s -0.003932 °C/s -0.003809 °C/s
124.1 J
MgO
-5316.4 J
3
0.4939 g
0.0123 mol
46.52 s
29.791 °C
33.51 °C
33.33 C
3.54 °C
1481.136 J
(1.48 kJ)
35.4 J
-1516.5 J
Use the following to determine the enthalpy of formation of magnesium oxide:
Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂ (g)
MgO (s) + 2HCl (aq) → MgCl₂ (aq)+ H₂O (1)
H₂(g) + ½O2 (g) → H₂O (1)
0.5033 g
MgO
0.0125 mol
32.47 s
31.5714 °C
35.27 °C
35.15 °C
3.59 °C
1502.056 J
(1.50 kJ)
35.9 J
-1538.0 J
-517.3 kJ/mol -506.3 kJ/mol -123.3 kJ/mol -123.0 kJ/mol
AH = (calculated in the experiment)
AH = (calculated in the experiment)
AH=285.8 kJ/mol
AH = (determine using Hess's Law)
Transcribed Image Text:Calculations:
1. Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of
liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide.
Show your work. If you are including a scan of your handwritten work, it must be legible.
2. Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of
percent error. Use the standard equation for this: |
%error
|actual value — experimental value|
|actual value|
x 100%
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