A 1.00g sample of octane (C8H18) is burned in a calorimeter that contains 1.20kg of water. The temperature of the water and the bomb rises from 25.00oC to 33.20oC. If the heat capacity of the bomb, Cbomb, is 837J/K calculate the heat given off per mole of octane. Specific heat for water: 4.184 J/g.°C
Please show work, correct equation to use and values. I know how to calculate heat but not sure how to correctly find heat per mole.
86 kJ/mol; 41.2 kJ/mol; 5.48 x 103 kJ/mol; 48.0 kJ/mol; 4.21 kJ/mol
Heat released by combustion of octane = heat gained by water + heat gained by calorimeter
Heat gained by calorimeter = C(cal) * ∆T
= 837*(33.20-25)
= 6863.4 joule or 6.863 KJ
Heat gained by water
= Mass * specific heat * ∆T
= ( 1.20*10^3)*4.184*(33.2 -25)
= 41170.56 joule or 41.171 KJ
Total heat = 41.171 + 6.863
= 48.034 KJ
Moles of octane = mass / molar mass
= 1/ 114
= 8.772*10^-3
8.772*10^-3 mole produces = 48.034 KJ
1 mole will produce = 48.034 / (8.772*10^-3)
= 5.475 *10^3 kJ / mol
Option C
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