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Heat Of Combustion Of Solid Magnesium Using Hydrochloric Acid And Magnesium Oxide In A Calorimeter. Ap Chemistry Lab Report

634 words - 3 pages

Heat of Combustion: Magnesium
In this experiment, you will use Hess’s law as you determine a heat of a reaction that would be
difficult to obtain by direct measurement—the heat of combustion of magnesium ribbon. The
reaction is represented by the equation:
Mg(s) + 1/2 O​2​(g) → MgO(s) This is the target equation.
This equation can be obtained by combining equations (1), (2), and (3):
(1) MgO(s) + 2 HCl(aq) → MgCl​2​(aq) + H​2​O(l)
(2) Mg (s) + 2 HCl(aq) → MgCl​2​(aq) + H​2​ (g)
(3) 2H​2​(g) + O​2​(g) → 2H​2​O(l) ΔH for this reaction ​-571.6 kJ.
In this experiment heats of reaction for equations (1) and (2) will be determined.
Pre-lab exercise
In the space provided below, “​rewrite”​ and combine equations (1), (2), and (3) to obtain the desired
target equation.
(1) ​MgCl​2​(aq) + H​2​O(l) → MgO(s) + 2 HCl(aq)
(2) ​Mg (s) + 2 HCl(aq) → MgCl​2​(aq) + H​2​ (g)
(3) ​H​2​(g) + 1/2 O​2​(g) → H​2​O(l)
Target:​ ​Mg(s) + 1/2 O​2​(g) → MgO(s)
Procedure: ​Bullet points or numbered list. Concise. Including amounts of chemicals used.
Graphs imported from logger pro: BELOW
1
Heat of Combustion: Magnesium
With Magnesium Oxide:
With Magnesium:
2
Heat of Combustion: Magnesium
Materials available
Go-Temp Probe 1.00 M HCl
styrofoam cup/calorimeter magnesium oxide, MgO no more than 2 g
utility clamp and stand etc Mg ribbon, no more than 1.0 g
graduated cylinders stirring rod
beakers weighing cup(s)
massing balance laptop computer
Data Colection: measured values only
Reaction 1
(MgO)
Reaction 2
(Mg)
Mass of Sample (Mg or
MgO)
1.49g 0.72g
Volume of HCl used 100mL 100mL
Mass of Styrofoam Cup 7.92g 7.92g
Mass of Cup + HCl 108.30 107.61
Accounting for Energy Loss:
● Real Temperature Change = slope * 0.5 * ^Time
○ Time it took to get to highest temperature
Data procesing:
a. Temperature correction: ​explanation and calculations
The temperature must be corrected to account for the heat lost...

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