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
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Chapter1: Chemical Foundations
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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)
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 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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