What volume of fuel should you bring? Assume each of the following: the fuel has

Question

What volume of fuel should you bring? Assume each of the following: the fuel has an average formula of 15 of the heat generated from combustion goes to heat the water (the rest is lost to the surroundings); the density of the fuel is 0.78 the initial temperature of the water is 25.0 and the standard enthalpy of formation of is -224.4 .

Explanation / Answer

-224.4 kJ/mole vs -44.566MJ/kg is a BIG difference. I thought 224 kJ for combustion was small but did not check it out earlier. Let UNITs guide you; always USE THEM in your calculation to prevent errors Firstly, the eqn: C7H16 + 11O2 -----> 7CO2 + 8H2O + heat dH comb/ mole C7H16 = 44.566 MJ /kg C7H16 = 44.566 kJ/g dH comb J /ml C7H16 = 44.566kJ/ g * 0.78 g/ml = ?? 34.76 kJ/ml heat needed, if 100% eff = 36000 g * 4.184 J/gC * 75 C = ?? 11.3 MJ if 15% eff then heat needed = 100% eff/15% * heat needed if 100% = 75.3 MJ vol of C7H16 needed = heat needed / (+dH comb / ml C7H16) = 75.3 MJ / 34.76 kJ/ml ?? 2167 ml liters C7H16 needed = vol ml / 1000ml/liter = ?? 2.17 liters 1 liter = 0.26 US gal; so 2.17 liters * 0.26 gal/liter = 0.56 gal Plug and SOLVE Basic mathematics is a prerequisite to chemistry – I just try to help you with the methodology of solving the problem.

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