The given reaction at top is not fully balanced it must have 8H2O
LUCJLIUILI Calculate the AH°rxn (in kJ) for combustion of acetone (C3HO): 2C3H6O(g) + 9O2(g) — 6CO2(g)...
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.
Example Problem Calculate the enthalpy (AH°, ) of combustion of Benzene, CH6. rxn C6H615/2 O2 (8)6CO2 (g) + 3H2O AH°, [C6H6= 49.0 kl/mol AH°% [CO2(@)= -393 .5 kJ/mol AHO, [H20 = -285.8 kl/mol AH', [O2@= 0 kl/mol
The standard enthalpy change for the combustion of 1 mole of propane is -2043.0 kJ. CzH3(g) + 5 O2(g) + 3 CO2(g) + 4H2O(g) Calculate 4, Hº for propane based on the following standard molar enthalpies of formation. molecule CO2(g) H2O(g) 4,Hº (kJ/mol-rxn) -393.5 -241.8
Calculate the AH formation of octane, CBH1B (), given that the enthalpy of combustion of octane is -5471 kl/mol and the standard enthalpies of formation of H20 () and CO2 (g) are -393.5 kJ/mol and -285.8 kJ/mol respectively.
Combustion of 2.5000 g of propane (C3H8) releases 115.75 kJ of heat when it is burned to form CO2 (g) and H2O (l). The standard formation enthalpies of CO2 (g) and H2O (l) are -393.5 kJ/mol and -285.5 kJ/mol respectively. Calculate the Hrxn for the combustion of propane in kJ/mol Calculate ∆?? ? for propane
A scientist measures the standard enthalpy change for the following reaction to be 2752.8 kJ : 6CO2(g) + 6H2O(1) C6H12O6 + 6 O2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH1:05 is kJ/mol A scientist measures the standard enthalpy change for the following reaction to be 53.9 LJ: CO2(g) + H2(g)— CO(g) + H2O() Based on this value and the standard enthalpies of formation for the other...
Question 2 (1 point) Saved The standard heat of combustion for naphthalene, C10Hg(s), is -5156.8 kJ mol-1. Use this value and the given standard enthalpies of formation to calculate the standard enthalpy of formation of C1oHg(s) in kJ mol-1 H20() AHOf: H20() -285.9 kJ mol-1; -285.9 kJ mol-1. CO2(g) = -393.5 kJ mol-1 Hint: Hess' law; write the balanced chemical combustion equation and the chemical equation which defines the AHf of C10H8(s).
e. -413.5 kJ = [71-52.7) + 3(-7-6 -25(15.) + -00- - 583.7 .180.7 17. The standard enthalpy of combustion for naphthalene, C H , (s), is -5156.8 kJ mol-1. Using this data and the standard enthalpies of formation, AH : H2O(l) = -285.9 kJ mol-1; CO2 (g) = -393.5 kJ mol-1, calculate the standard enthalpy of formation of Co H, (s), in kJ mol-1. a. +78.2 kJ b. +935.9 kJ c. -1065.4 kJ d. +3619.7 kJ e. -10235.4 kJ
2. Given the following heats of formation, calculate AH for the reaction 2 CO(g) + 5 H2(g) → C2H6 (g) + 2 H2O(g) Compound AH°F (kJ/mol) Compound AH°F (kJ/mol) 52.28 C₂H6 (8) -84.68 C2H4 (8) -393.5 CO2(g) -241.8 H2O(g) -285.9 CO(g) -110.5 H2O(1)
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