The combustion of 2.034 g of propanol ( C 3 H 7 OH ) increases the temperature of a bomb calorimeter from 298.00 K to 302.88 K . The heat capacity of the bomb calorimeter is 13.99 kJ/K . Determine Δ H for the combustion of propanol to carbon dioxide gas and liquid water.
use:
Q cal = Ccal*delta T
Q cal = 13.99*(302.88-298.0)
Q cal = 68.27 KJ
This heat is supplied by C3H7OH
Molar mass of C3H7OH,
MM = 3*MM(C) + 8*MM(H) + 1*MM(O)
= 3*12.01 + 8*1.008 + 1*16.0
= 60.094 g/mol
mass(C3H7OH)= 2.034 g
use:
number of mol of C3H7OH,
n = mass of C3H7OH/molar mass of C3H7OH
=(2.034 g)/(60.09 g/mol)
= 3.385*10^-2 mol
use:
delta H = -Qcal/number of mol
= -68.27 KJ / 3.385*10^-2 mol
= -2.017*10^3 KJ/mol
Answer: -2.02*10^3 KJ/mol
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