Question #118823
calculate the molar enthalpy of the combustion of butane if 1.22 g of the fuel increased the temperature of a tin can calorimeter (22.5 g of tin and 200 mL of water) by 8.30 celsius
1
Expert's answer
2020-06-02T14:07:41-0400

The molar enthalpy of the combustion is the amount of energy released when 1 mole of the substance combusts in excess oxygen:

H=Q/nC4H10∆H = -Q/n_{C_4H_{10}} .

The energy released can be calculated using the specific heat capacities of tin ctinc_{tin} ​ (0.218 J/g°C) and of water cwc_w (4.186 J/g°C). Assuming the density of water equal 1 g/mL, the mass of water is 200 g. Therefore:

Q=(ctinmtin+cwmw)TQ = (c_{tin}m_{tin}+c_{w}m_w)∆T

Q=(0.21822.5+4.186200)8.30=6.99103Q = (0.218·22.5+4.186·200)·8.30 = 6.99·10^3 J.

The number of the moles of butane is its mass divided by its molar mass (58.12 g/mol):

n=m/M=1.22/58.12=0.0210n = m/M = 1.22/58.12 = 0.0210 mol.

Finally, the molar enthalpy of combustion of butane is:

H=6.991030.0210=3.33105∆H = -\frac{6.99·10^3}{0.0210} = 3.33·10^5 J/mol, or 333 kJ/mol

Answer: the molar enthalpy of the combustion of butane is 333 kJ/mol.


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