Solution:
The enthalpy of combustions and heat capacities are given
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
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...
The standard enthalpy of combustion of cyclopropane is -2091 kJ/mol at 298 K. The enthalpy of formation of CO_2 (g) and H_2 O (I) are -393 kJ/mol and -286 kJ/mol, respectively. Calculate the enthalpy of formation of cyclopropane Given that the enthalpy of formation of propene is 20.42 kJ/mol, please calculate the enthalpy of isomerization of cyclopropane to propene.
CO2(g) H2O(g) CH4(g) +17 AHp/kJ mol -394 -242 These data can be used to calculate the enthalpy change for the reaction in part (b). (ii) Use the data from the formation table above to calculate the standard enthalpy of combustion of methane. 13 marke
7. The enthalpy of combustion of C to CO2 is –393.5 kJ/mol C, and the enthalpy of combustion of Co to CO2 is -283.0 kJ/mol CO: C(s) + O2(g) + CO2(g) AH = -393.5 kJ CO(g) + 102(9) CO2(g) AH = -283.0 kJ Using these data, calculate the enthalpy of combustion of C to CO: C(s) + O2(g) → CO(g) AH = ? Answer: -110.5 kJ
AU for the reaction CH4 (8) + 2O2(g) - CO2(8) + 2H2O(l) in kJ at 298 K is AH(CH,) =-74.6kJ / mol AH (0) = -393.5kJ / mol AH,(4,0) =-285.8kJ / mol 1 A. -885.5 kJ B.668 kJ C. 885.5 kJ D.-668 kJ
), is determined to be -7835.7 kJ mol!! The standard enthalpy change of combustion [to CO2(g) and H200) at 25°C of the organic solid pyrene, CH What is the AH of C16H10(s) based on this value? Use the following data: AH? H20 () --285.83 kJ moll: AH? CO2(8) --393.51 kJ mol! kJ mol!
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l) ΔΗ =-890.3 kJ 1. Calculate the AH when 5.00 g CH4 react with excess of oxygen. 2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen 3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid para-benzoquinone, C6H4O2(s), is determined to be -2767.0 kJ mol-1. What is the Hf° of C6H4O2(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 kJ mol-1
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid bianthracene, C28H18(s), is determined to be -13924.1 kJ mol-1. What is the Hf° of C28H18(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 _________ kJ mol-1
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).