Water mass 100.0 mL of pure water. heat capacity of the calorimeter as 10.0 J/ºC Room TemperatureReactantTrial NumberMass 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-TiqwatercalorimeterqrxuAHrxn26.0°CMg (s) + O2 (g) → MgO (s)Mg10.2578 g33.5 s24.3°CMg37.23 °C20.2551 g41.05 s29.055 °CMgO41.72 °Cun30.4939 g46.52 s29.791 °C33.51 °CUse 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 (l)-0.005191 °C/s -0.006452 °C/s -0.003932 °C/s -0.003809 °C/sMgO0.5033 g432.47 s31.5714°CAH = (calculated in the experiment)AH = (calculated in the experiment)ΔΗ- 285.8 kJ/mol35.27 °CAH = (determine using Hess's Law)

qwater = (mass of water used) x 4.184 J/g-ºC x (Tf – Ti) qcalorimeter = 10.0 J/ºC x (Tf – Ti) Mass…

Answered: Room Temperature Reactant Trial Number…

Room Temperature Reactant Trial Number Mass of reactant (from data) 26.0°C Mg 1 0.2578 g Mg 2 0.2551 g MgO 3 0.4939 g MgO 4 0.5033 g

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.16PAE: 9.16 According to Figure 9.2, the total energy supply in the United States in 2016 was 111.261015...

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Question

100%

Water mass 100.0 mL of pure water.

heat capacity of the calorimeter as 10.0 J/ºC

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
qwater
calorimeter
qrxu
AHrxn
26.0°C
Mg (s) + O2 (g) → MgO (s)
Mg
1
0.2578 g
33.5 s
24.3°C
Mg
37.23 °C
2
0.2551 g
41.05 s
29.055 °C
MgO
41.72 °C
un
3
0.4939 g
46.52 s
29.791 °C
33.51 °C
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 (l)
-0.005191 °C/s -0.006452 °C/s -0.003932 °C/s -0.003809 °C/s
MgO
0.5033 g
4
32.47 s
31.5714°C
AH = (calculated in the experiment)
AH = (calculated in the experiment)
ΔΗ
- 285.8 kJ/mol
35.27 °C
AH = (determine using Hess's Law)

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