Question

If a lighter contains 4.0 mL of liquid butane (density of butane - 0.8 g/cm), how much heat can we get out of it from the combustion of butane? 2 C.Hole) + 13 O2(g) + CO2(g) + 10 H2O(1) 4H -5.75 X 10 kJ/mol 16x 10k) 8x 10? 5x 10 kJ 4.8* 10 kJ What is the physical property of a material that measures how much heat is required to raise the temperature of 1 mole of that material by 1°C? specificheat capacity molar heat of fusion specific heat of heating molar heat capacity The following reaction can be characterized as a(n) CH4(g) + 2 02(8) CO2(g) + 2 H2O(1) AH --890.4 kJ/mol reduction reaction exothermic reaction displacement reaction endothermic reaction A calorimeter is used to compare the energy content of some fuels. During the calibration of the calorimeter, an electrical resistance heater supplies 120 J of heat and a temperature increase of 0.920°C is observed. Then, 0.3 g of a particular fuel is burned in this same calorimeter, and the temperature increases by 6.15°C. What is the amount of energy liberated per one gram of fuel burned? 4.1kJ 3.2 kJ 5.7) 2.7kJ

Answer 1

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Volume of butane - 4.0 ml: density of butane = 0.8 g/cm3. os mass of boutane = Volume x density = 400 ml x 0.8 g/ml = 302 g Molar mass butane = 58 g/mol los moles of butane = mass molar mass = 302 mol OH = - 5•75 x 103 kJ/mol 58mb4 - 0noH = 3:2 x 5.75 x 709 KJ 582 = 126 X 102 IJ Here, it is devided by ? because stochiometary of CtHio is lo Molar heat_capacity 3 Exothermic reaction: _ Heat is evolved as oH is negative for calibiration ΔΤ 120 1.20 - 0 + 02 3_802.17 I oo 003 g fuel gives 802017 J CS Lamscanner . i " 802.17 J = 2.7 kJ 03