When 0.1523 g of liquid pentane (C5H12) combusts in a bomb calorimeter, the temperature rises from 23.7∘C to 29.8 ∘C. What is ΔUrxn for the reaction in kJ/mol pentane? The heat capacity of the bomb calorimeter is 5.23 kJ/∘C.
Q cal = Ccal*delta T
= 5.23 KJ/oC*(29.8-23.7)oC
= 31.903 KJ
This heat is supplied by pentane
Molar mass of C5H12 = 5*MM(C) + 12*MM(H)
= 5*12.01 + 12*1.008
= 72.146 g/mol
mass of C5H12 = 0.1523 g
we have below equation to be used:
number of mol of C5H12,
n = mass of C5H12/molar mass of C5H12
=(0.1523 g)/(72.146 g/mol)
= 2.111*10^-3 mol
delta U = -Qcal/number of mol
= -31.903 KJ / 2.111*10^-3 mol
= -15113 KJ/mol
Answer: -15113 KJ/mol
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