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
Use the following data to calculate the standard enthalpy of formation of heptane, C7H16 (l). C7H16...
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...
Use the following data to calculate the standard enthalpy of formation of solid strontium carbonate SrCO3 (s) → SrO (s) + CO2(s) ΔH° = 234 kJ/mol ΔHf° of CO2 (g) = -394 kJ/mol ΔHf° of SrO(s) = -592 kJ/mol A) -752 kJ B) 752 kJ C) -1220 kJ D) -1812 kJ E) 1812 kJ f) 1220
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
What is the standard enthalpy of formation of What is the standard enthalpy of formation of CH 3 CH 2 CH 2 CHO(l)? CH3CH2CH2CHO(l)? 2CH 3 CH 2 CH 2 CHO(l)+5O 2 (g)→8H 2 O(l)+8CO 2 (g); 2CH3CH2CH2CHO(l)+5O2(g)→8H2O(l)+8CO2(g); ΔH°=–4943.6 kJ ΔH°=–4943.6 kJ Substance ΔH° f (kJ/mol) CO 2 (g) -393.5 H 2 O(l) –285.8 a. –245.4 kJ/mol b. +245.4 kJ/mol c. –1792.5 kJ/mol d. –3151.1 kJ/mol e. +3151.1 kJ/mol
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, Δ H o f 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
PROBLEM-SOLVING CLASS ACTIVITY 11 Use Hess's Law to calculate the enthalpy of formation of CH2OH: C(graphite) + 2 H2(g) + 1026) → CH2OH(1) Given the following data: CH2OH() • 02(9) + CO2(g) + 2H2O(1) AH°: -726.4 kJ/mol C(graphite). O2(g) → CO2(9) AH' = -393.5 kJ/mol H2(g) + 40269) → H2O(1) AH = -285.8 kJ/mol
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.
Use the following information to calculate the heat of formation of propane C3H8. 3 C (S-Graphite) + 4 H2 (g) —› C3H8 (g) 1. C (S-Graphite) + O2 (g) —› CO2 (g) ΔH = - 393.5 kJ 2. H2 (g) + ½ O2 (g) —› H2O (l) ΔH = - 285.8 kJ 3. C3H4 (g) + 4 O2 (g) —› 3 CO2 (g) + 2 H2O (l) ΔH = - 1937 kJ 4. C3H6 (g) + 9/2 O2 (g) —›...
help asap 3. Calculate the standard enthalpy change, Hº, for the following reaction using standard enthalpies of formation. (1 point) 2C2H2(g) + 502(g) → 4CO2(g) + 2H20(1) Standard Enthalpies of Formation AH for C2H2(g) = +226.7 kJ/mol AHfor CO2(g) = -393.5 kJ/mol AH for H2O(l) = -285.8 kJ/mol
Heat of Formation Calculations: 32) Use a standard enthalpies of formation (Ho) table to determine the change in enthalpy for each of these reactions Hrxn [n. Ho(products) - n. Ho(products)] CO (g): -110.5 kJ/mol; CO2 (g): -393.5 kJ/mol CH4 (g): -890.4 kJ/mol H2O (l): -285.8 kJ/mol; H2O (g): -241.8 kJ/mol H2S (g): -20.6 kJ/mol; NO: -90.2 kJ/mol NO2: +33.9 kJ/mol; HCl (g): -92.3 kJ/mol NaOH (s): -426.7 kJ/mol; SO2 (g): -296.8 kJ/mol a) CH4(g) + 2 O2(g) ---> CO2(g) +...