The complete combustion of propane, C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4 H2O(l) has DH = -2220 kJ. How much heat is evolved in the complete combustion of 20.0 L C3H8(g) at 1 atm pressue and 0 oC? A) 2486 kJ B) 1007 kJ C) 994 kJ D) 1957 kJ E) 495 kJ

The value of AH° for the reaction below is 128.1 kJ CH,OH -Co, + 2H (1) 2(g) 2(g) How may kJ of heat are consumed when 10.1 g of H2(g) is formed as shown in the equation? Given that the atomic mass of C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol Show your answers in TWO (2) decimal places. Do not include the units in your final answers.

4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise (AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (C,) of 5.500 kJ/°C. o Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas in the calorimeter Яр [ Select ] kJ / 3.500 g of C4H10 o Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas): C4H10(9) + 13/2 02(9) → 4 CO2(9) + 5 H20(g) AHrxn [ Select ] kJ / mol of C4H10 • Use the heats of formation (AH¢°) to calculate the change in enthalpy (AHrxn) for the same reaction. (for 1 mole of butane gas): Heats of Formation: CO2 (g) - A H°f = -393.5 kJ/mol H2O(g) - A H°f = -241.8 kJ/mol O2 (9) - A H°f 0.0 kJ/mol C4H10 (g) - A H°f = -125.6 kJ/mol C4H10(g) + 13/2 02(g) → 4 CO2(9) + 5 H20(g) ΔΗη [ Select ] kJ / mol of C4H10

The oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/mol