Question

select an article that details current methods that are used to successfully prevent identity theft. Discuss what

security policies commerce should implement to prevent it from happening. Also, address the options users can take to protect themselves.

 

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Question

1.  Record the following for each of the three trials:
·  Trial

1

a	Mass of the empty calorimeter (g)18.6g
b	Initial temperature of the calorimeter (°C)21.5°C
c	Maximum temperature in the calorimeter from the reaction (°C)35.0°C
d	Calculate ΔT by subtracting (b) from (c) (°C) ΔT = Tmaximum – Tinitial35.0°C-21.5°C=13.5°C
e	Mass of the calorimeter and its contents after the reaction (g)68.74g
f	Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)68.74g-18.6g=50.14g
g	Calculate the moles of Mg reacted (MW = 24.305 g/mole)?50mL of 1M HCI is 50/1000×1=0.05.15/24.305=.006g/mole

·  Trial 2

a	Mass of the empty calorimeter (g)18.6g
b	Initial temperature of the calorimeter (°C)21.5°C
c	Maximum temperature in the calorimeter from the reaction (°C)44.0°C
d	Calculate ΔT by subtracting (b) from (c) (°C) ΔT = Tmaximum – Tinitial44.0°C-21.5°C=22.5°C
e	Mass of the calorimeter and its contents after the reaction (g)68.83g
f	Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)68.83-18.6=50.23
g	Calculate the moles of Mg reacted (MW = 24.305 g/mole).25/24.305=.010g/mole

·  Trial 3

a	Mass of the empty calorimeter (g)18.6g
b	Initial temperature of the calorimeter (°C)21.5°C
c	Maximum temperature in the calorimeter from the reaction (°C)52.9°C
d	Calculate ΔT by subtracting (b) from (c) (°C) ΔT = Tmaximum – Tinitial52.9°C-21.5°C=31.4°C
e	Mass of the calorimeter and its contents after the reaction (g)68.92g
f	Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)68.92g-18.6g=50.32
g	Calculate the moles of Mg reacted (MW = 24.305 g/mole).35/24.305=.014g/mole

2.  Calculate the heat released into the solution for the 3 reactions, according to the formula:

qreaction= (Ccal * ΔT) + (mcontents* Cpcontents* ΔT)

3.  
Assume Cp_contents= Cp_water= 4.18 J/g °C

a	Trial 1 (J)(4.18J/g°C)(68.74g)(35.0°C-21.5°C)=3878.9982 J/g°C
b	Trial 2 (J)(4.18J/g°C)(68.83g)(44.0°C-21.5°C)=6473.4615 J/g°C
c	Trial 3 (J)(4.18J/g°C)(68.92g)(52.9°C-21.5°C)=9045.88784 J/g°C

4.  Find the molar heat of reaction for each experiment in units of kilojoules / (mole of Mg) by dividing the heat of reaction (converted to kJ by dividing by 1000) by the moles of Mg used.

a	Trial 1 (kJ/mol)
b	Trial 2 (kJ/mol)
c	Trial 3 (kJ/mol)

5.  Calculate and record the average molar heat of reaction from the three results:

 

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