Question

The heats of combustion of ethane (C2H6) and butane (C4H10) are 52 kJ/g and 49 kJ/g, respectively. We need to produce 1.000 x 103 kJ heat by burning one of the fuels. Which fuel will emit the least amount of CO2? 1. Calculate the number of grams needed of each fuel: 2. Calculate the number of moles of each fuel: 3. Write down the balanced chemical equation for the combustion of the fuels: 4. Calculate the number of moles of CO2 produced by burning each fuel to produce 1.000 x 103 kJ. Which fuel will emit the least amount of CO2?

Answer 1

Now we need to produce 1.000810 kJ = 1000kJ 1. For 52 kJ energy, amount of C MG required= lg so for 1000 kJ energy, amount of Cal required = 1 x loog = 19.239 For 49 kJ, heat, amount of Cu Mio required = lg so for 1000 kJ heat, amount of Culio required = 1 X 1000 = 201408g

2. moles of C₂M6 = massa Cato masa (g) olar mass (almall 19.23g = 0.64lmol 30g/mol molen of Cumro = 20.408 g = 0.3519 mol 58 g/mol -3. C₂ Morgo + 2 02(g) → 2CO2 (g) + 3H₂O(g) Cu Mio Lg + 12 OR cgj 4CO2(g) + SH2O (g) 4. molex of co from 0.641 mol of C₂Mo = 2X0.641 = 1.282 mol molen of co, from 0.3519 mol of Culio = 4x0.3519 = 1.4076 So Cato is emitting least amount of Co,