Given the following thermochemical data, what is the standard enthalpy of combustion of C2H6 in kJ·mol–1?
H2 (g) + 1/2 O2 (g) → H2O (l) | ΔH0= –286 kJ |
C2H4 (g) + H2 (g) → C2H6 (g) | ΔH0= –137 kJ |
C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (l) | ΔH0= –1412 kJ |
Given the following thermochemical data, what is the standard enthalpy of combustion of C2H6 in kJ·mol–1?...
The standard enthalpy of combustion of ethane gas, C2H6 is −1560 kJ·mol−1. Given that ∆Hf° CO2, (g) = −394 kJ·mol−1, and ∆Hf° H2O, (l) = −286 kJ·mol−1. Calculate ∆Hf° C2H6 (g).
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...
3. Calculate the standard enthalpy change (AHº) for the combustion of methane given the following data: AH° = -232.4 kJ CH4(g) + O2(g) → CH2O(g) + H20 (g) CH20 (g) + O2(g) → CO2(g) + H2O(g) AH° = -343.5 kJ 3. Calculate the standard enthalpy change (AHº) for the combustion of methane given the following data: AH° = -232.4 kJ CH4(g) + O2(g) → CH2O(g) + H20 (g) CH20 (g) + O2(g) → CO2(g) + H2O(g) AH° = -343.5 kJ...
Isooctane C8H18 is a major component of gasoline. Determine the change in enthalpy for the combustion of 228.0 g of isooctane from the following data: H2 (g) + 1/2O2 (g) ⟶ H2O (g) ΔH0 = −241.8 kJ C (s) + O2 (g) ⟶ CO2 (g) ΔH0 = −393.5 kJ 8C (s) + 9H2 (g) ⟶ C8H18 (l) ΔH0 = −224.13 kJ
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
Calculate the standard enthalpy of formation of gaseous carbon dioxide (CO2) using the following thermochemical information: 2 C(s) + H2(g) C2H2(g) H = +226.8 kJ 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(l) H = -2599.3 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ H = _______kJ
Calculate the standard enthalpy of formation of gaseous acetylene (C2H2) using the following thermochemical information: 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(l) H = -2599.3 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ H = kJ
Calculate the standard enthalpy of formation of gaseous methane (CH4) using the following thermochemical information: CO2(g) + 2 H2O(l) CH4(g) + 2 O2(g) H = +890.4 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ
Calculate the standard enthalpy of formation of liquid water (H2O) using the following thermochemical information: CH4(g) C(s) + 2 H2(g) H = +74.8 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ CO2(g) + 2 H2O(l) CH4(g) + 2 O2(g) H = +890.4 kJ
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...