Answer:
a. -538 kJ/mol
Explanation:
Internal energy change (ΔU) for the reaction of combustion in the bomb calorimeter is:
ΔU = q calorimeter + q solution
Where:
q calorimeter is Ccal×ΔT, (Ccal=3,81kJ/°C) and (ΔT is 0,285°C)
q solution is c×m×ΔT (c= 4.184 J/g°C), (m=3000g H₂O), (ΔT is 0,285°C)
Replacing:
ΔU = 1,09kJ + 3,58kJ = 4,67 kJ
This energy is per 0,485g of X, now, per mole of X
[tex]\frac{4,67kJ}{0,485gX} *\frac{56,0g}{1mol}[/tex]= -539kJ/mol ≡ a. -538 kJ/mol
-negative because the energy is produced by rising of temperature-
I hope it helps!
Answer:
For 56 g/mol of compound the change in the internal energy is found to e -539 kJ/mol.
Explanation:
[tex]\rm \Delta[/tex]U for a reaction is the internal energy change in the reaction. For a reaction in the bomb calorimeter,
[tex]\rm \Delta[/tex]U = Heat of calorimeter + Heat of solution
Heat = Heat capacity [tex]\times[/tex] Temperature
For, 0.485 g compound
[tex]\Delta[/tex]U = 3.81 [tex]\times[/tex] 0.285 + 4.184 [tex]\times[/tex] 3000 [tex]\times[/tex] 0.285
[tex]\Delta[/tex]U = 4.67 kJ
For 56 g/mol compound:
[tex]\Delta[/tex]U = [tex]\rm \frac{energy}{mass}\;\times\;\frac{moles}{1}[/tex]
[tex]\Delta[/tex]U = [tex]\rm \frac{4.67}{0.485}\;\times\;56[/tex]
[tex]\Delta[/tex]U = 539 kJ/mol
Since there is rise in temperature in the reaction, the negative sign is imparted to the internal energy, i.e. -539kJ/mol.
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