What is the standard enthalpy change for the combustion of gaseous propylene, C3H6? C3H6(g) + 9/2 02(g) → 3CO2(g) + 3H20(1) C3H6(g) AH°f (kJ/mol) +20.4 CO2(g) AH°f (kJ/mol) -393.5 H20(1) AH°f (kJ/mol) -285.8 O a. +2017.5 kJ O b. +2058.3 kJ O C. -2017.5 kJ O d. -2058.3 kJ e. -658.9 kJ

When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?

The heat capacity of a bomb calorimeter was determined by burning 6.85 g of methane (energy of combustion = -803 kJ/mol CH4) in the bomb. The temperature changed by 11.1°C. (a) What is the heat capacity of the bomb? kJ/°C (b) A 14.7-g sample of ethanol (C₂H5OH) produced a temperature increase of 12.8°C in the same calorimeter. What is the energy of combustion of ethanol (in kJ/mol)? kJ/mol

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic     (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =  kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1