Calculate enthalpy of combustion of acetone, C3H6O, given the following information:
(ΔH°f [ C3H6O(g)] = -285 kJ/mol
(ΔH°f [ CO2(g)] = -394 kJ/mol
(ΔH°f [ H2O(ℓ)] = -286 kJ/mol
Answer choices.....
A)-2613 kJ
B) -395 kJ
C) -1755 kJ
D) -585 kJ
E) -965 kJ
Calculate enthalpy of combustion of acetone, C3H6O, given the following information: (ΔH°f [ C3H6O(g)] = -285...
The enthalpy of combustion (ΔH°c) of 1,1,2,2,-tetramethylcyclopropane (C7H14) is -4635.62 kJ/mol. a-Using the appropriate information given below, calculate the enthalpy of formation (ΔH°f), in kJ/mol, for 1,1,2,2,-tetramethylcyclopropane. Report your answer to two decimal places. ΔH°f (CO2 (g)) = -393.51 kJ/mol ΔH°f (H2O (l)) = -285.83 b- Determine the mass (in g) of 1,1,2,2,-tetramethylcyclopropane produced, if ΔH° was determined to be -35.93 kJ during an experiment in which 1,1,2,2,-tetramethylcyclopropane was formed. Report your answer to three significant figures.
LUCJLIUILI Calculate the AH°rxn (in kJ) for combustion of acetone (C3HO): 2C3H6O(g) + 9O2(g) — 6CO2(g) + 6H2O(1) The standard enthalpies of formation are: CO2(g) AH°F = -393.5 kJ/mol H2O(1) AHºr=-285.9 kJ/mol C3H6O(g) AH° = -216.6 kJ/mol
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...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
Calculate the standard enthalpy of reaction for the combustion of propane. NOTE: This equation is not balanced. Round to the nearest whole number. C3H8(g) + O2 --> CO2(g) + H2O(l) kJ/mol Compound Hf (kJ/mole) C3H8(g) -105 CO2(g) -394 H2O(l) -284
calculate the enthalpy of the combustion of propane for your barbeque C3H8 + 5O2 -> 3CO2 + 4H2O propane -105 kJ/mol CO2 -394 kJ/mol Water -286 kJ/mol Ooxygen. 0
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 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...
Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ Express your answer with the appropriate units. Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ Express your answer with the appropriate units.