The compound heptane, C7H16, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is C7H16(ℓ) + 11 O2(g)7 CO2(g) + 8 H2O(g)
The standard enthalpy of formation of liquid heptane at 25 °C is -224.2 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C7H16(g) = -187.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8
(a) Calculate the enthalpy change in the burning of 2.000 mol liquid heptane to form gaseous products at 25°C.
State explicitly whether the reaction is endothermic or exothermic. ΔH° = kJ (b) Would more or less heat be evolved if gaseous heptane were burned under the same conditions?
What is the standard enthalpy change for vaporizing 2.000 mol C7H16() at 25°C? ΔH° = kJ
Calculate the enthalpy change in the burning of 2.000 mol gaseous heptane to form gaseous products at 25°C. ΔH° = kJ
The compound heptane, C7H16, is a good fuel. It is a liquid at ordinary temperatures. When...
The compound 1-pentanol, C5H12O, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C5H12O(ℓ) + 15 O2(g)10 CO2(g) + 12 H2O(g) The standard enthalpy of formation of liquid 1-pentanol at 25 °C is -351.6 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C5H12O(g) = -294.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 5.000 mol...
The compound 1-propanol, C3H8O, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C3H8O(ℓ) + 9 O2(g)6 CO2(g) + 8 H2O(g) The standard enthalpy of formation of liquid 1-propanol at 25 °C is -302.6 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C3H8O(g) = -255.1 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 3.000 mol...
Use the following data to calculate the standard enthalpy of formation of heptane, C7H16 (l). C7H16 (l) + 11 O2 (g → 7 CO2 (g) + 8 H2O (l) ΔH° = -4817 kJ/mol ΔHf° of CO2 (g) = -393.5 kJ/mol ΔHf° of H2O (l) = -285.8 kJ/mol A)-218.2 kJ/mol B)-468.1 kJ/mol C)-223.9 kJ/mol D)-447.8 kJ/mol E)-111.5 kJ/mol
When styrene C8H8 burns in oxygen to form carbon dioxide and liquid water under standard-state conditions at 25°C, 42.62 kJ are released per gram of styrene. Find the standard enthalpy of formation of styrene at 25°C. (Given: ΔH°f[CO2(g)] = –393.5 kJ/mol, ΔH°f[H2O(l)] = –285.8 kJ/mol)
The gas ethane, C2H6(g), can be used in welding. When ethane is burned in oxygen, the reaction is: 2 C2H6(g) + 7 O2(g)4 CO2(g) + 6 H2O(g) (a) Using the following data, calculate ΔH° for this reaction. ΔH°f kJ mol-1: C2H6(g) = -84.0 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ΔH° = kJ (b) Calculate the total heat capacity of 4 mol of CO2(g) and 6 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...
A sample of liquid methanol weighing 5.27 g was burned in a bomb calorimeter at 25°C, and 119.50kJ of heat was evolved. a. Calculate AHº for the combustion of 1 mole of methanol. b. Calculate A/Hºof liquid methanol. A Hºof CO2(g), H2O(g) and H20 (1) are -393.5 kJ/mol, 241.8 kJ/mol, -285.8 kJ/mol, respectively (10 pt)
11. Kathleen burned heptane (C7H16) in the air: CH16 (1) + 1102(g) → 7CO2(g) + 8H2O(g). Which of the following is NOT correct for this reaction? a. 1 mol of C7H16 reacts with 11 mol of 02. b. C His is a liquid. c. CO is a gas. d. 1 mol of CyHo produces 7 mol of H2O. Answer:
Isooctane C3H18 is a major component of gasoline. Determine the change in enthalpy for the combustion of 2.000 mol of isooctane from the following data: H2(g) + (1/2)02(g) + H2O(g) AH° = –241.8 kJ C(s) + O2(g) + CO2(g) AH° = -393.5 kJ 8C (s) + 9H2(g) → CgH 18 (1) AH° = -224.13 kJ Isooctane CgH 18 is a major component of gasoline. Determine the change in enthalpy for the combustion of 2.000 mol of isooctane from the following...
Given: C(s) + O2(g) ---> CO2(g) ΔH = −393.5 kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = −296.8 kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = +87.9 kJ/mol A) Calculate the standard enthalpy change for the following reaction CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) ΔH° rxn = -1075 kJ/mol B) Using the equation and standard enthalpy change for the reaction (from part A), calculate the amount of heat produced or consumed when 3.2 mol of CS2 reacts with excess...
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol