Homework Answers
Chemical reaction for combustion of C8H18 is ;
2C8H18 + 25O2 = 18H2O + 16CO2 + heat (given -5471kJ/mol)
?H of reaction = sum of ?H°f of formation of products - sum of ?H°f formation of reactants .
2× -5471(as 2 moles ) = ( ?H°f 18 H2O + ?H°f 16 CO2 ) - ?H f of 2 Octane ( ?H°f of O2 is zero) .
?H°f of 2 Octane = [18 (-393.5) + 16 (-285.8)] - (-10942)
?H°f of 2 moles of Octane = - 11655.8 + 10942 = -713.8 kJ .
Now enthalpy of formation of octane(l) = -713.8/2 = -356.9 kJ/mole .
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Calculate the AH formation of octane, CBH1B (), given that the enthalpy of combustion of octane...
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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
I just want to see the steps on how to work out the problem, thanks. 18....
I
just want to see the steps on how to work out the problem,
thanks.
18. Octane (CHıx) undergoes combustion according to the following thermochemical equation. 2C3H13() + 2502(g) → 16CO2(g) + 18H2011 AHnx = -1.0940 * 10ºkJ/mol What is the standard enthalpy of formation of liquid octane? AH* (CO2(g)) = -393.5 kJ/mol and AH® (H20(0) = -285.8 kJ/mol A.-250 kJ/mol B. -10,940. kl/mol C.-2188 kJ/mol D. -495 kJ/mol E. 495 kJ/mol
help pt) A sample of 1.0 mol of liquid octane C8H18(1) undergoes combustion accord 5. (10...
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pt) A sample of 1.0 mol of liquid octane C8H18(1) undergoes combustion accord 5. (10 pt) A C3H18(0) + O2(g) → 8 CO2(g) + 9 H2O(l) Using the standard enthalpies of formation given calculate the change in enthalpy in kJ/mol associated with the combustion of 1.0 mol of C8H18(1) at 1.0 bar pressure and 25 °C. Substance AH® (kJ/mol) C8H18() -249.9 CO2(g) -393.51 H2O) -285.83
need help with 2. Use the following enthalpies of formation to calculate an approximate enthalpy of...
need help with
2. Use the following enthalpies of formation to calculate an approximate enthalpy of reaction, AHrxn for: (5 pts) C3H8 (g) + 502 (g) → 3CO2 (g) + 4 H20 (1) C(s) + O2 (g) - CO2 (g); AH = - 393.5 kJ/mol H2(g) + 42 02 (g) - H20 (1); AH = - 285.5 kJ/mol 3 C(s) + 4 H2(g) → C3H8 (g); AH r = - 103.8 kJ/mol
LUCJLIUILI Calculate the AH°rxn (in kJ) for combustion of acetone (C3HO): 2C3H6O(g) + 9O2(g) — 6CO2(g)...
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
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2...
5. Using standard heats of formation, calculate AH for 4 FeO (s) + O2(g) → 2 Fe2O3 (s) AH1 of FeO (s) = -272.0 kJ/mol AHºf of Fe2O3 (s) = -825.5 kJ/mol 3. Given 3 C (s) + 4 H2(g) → C3H8 (9) AH = -103.85 kJ/mol C(s) + O2(g) + CO2(g) AH = -393.5 kJ/mol H2 (g) + 12 O2(g) → H2O (1) AH = -285.8 kJ/mol find AH for C3H8 (g) + 5 O2(g) → 3 CO2 (g)...
58. Calculate the standard enthalpy of formation of PCI, (g), given that AH' = -136.0 ks...
58. Calculate the standard enthalpy of formation of PCI, (g), given that AH' = -136.0 ks for the reacti PCI, (g) + H2O(g) POCI, (g) + 2 HCI (8) and the following standard enthalpies of formation: H,0 (8), -241.8 kJ/mol; POCI, (), -592 kJ/mol; HCl (g), -92.5 kJ/mol.
7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s)...
7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s) + O2(g) + CO2(g) b. S(s) + O2(g) → SO2(e) C. CS2() + 302(g) → CO2(g) + ' 250 (6) AH° = -393.5 kJ/mol AH° = -296.4 kJ/mol AH° = -1073.6 kj/mol (the standard state of the element Sulfur is S(s))
The combustion of lauric acid is given by the following thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g)...
The combustion of lauric acid is given by the following
thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) +
12 CO2(g) Hcomb is −7377 kJ mol−1 Using the heats of formation
for CO2(g) and H2O(l) calculate the heat of formation (△fH) of
lauric acid. △fH△ CO2(g) = −393.5 kJ mol−1 fH
H2O(l)= −285.8 kJ mol−1
19. The combustion of lauric acid is given by the following thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) + 12 CO2(g) AH...
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
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
I
just want to see the steps on how to work out the problem,
thanks.
18. Octane (CHıx) undergoes combustion according to the following thermochemical equation. 2C3H13() + 2502(g) → 16CO2(g) + 18H2011 AHnx = -1.0940 * 10ºkJ/mol What is the standard enthalpy of formation of liquid octane? AH* (CO2(g)) = -393.5 kJ/mol and AH® (H20(0) = -285.8 kJ/mol A.-250 kJ/mol B. -10,940. kl/mol C.-2188 kJ/mol D. -495 kJ/mol E. 495 kJ/mol
help
pt) A sample of 1.0 mol of liquid octane C8H18(1) undergoes combustion accord 5. (10 pt) A C3H18(0) + O2(g) → 8 CO2(g) + 9 H2O(l) Using the standard enthalpies of formation given calculate the change in enthalpy in kJ/mol associated with the combustion of 1.0 mol of C8H18(1) at 1.0 bar pressure and 25 °C. Substance AH® (kJ/mol) C8H18() -249.9 CO2(g) -393.51 H2O) -285.83
need help with
2. Use the following enthalpies of formation to calculate an approximate enthalpy of reaction, AHrxn for: (5 pts) C3H8 (g) + 502 (g) → 3CO2 (g) + 4 H20 (1) C(s) + O2 (g) - CO2 (g); AH = - 393.5 kJ/mol H2(g) + 42 02 (g) - H20 (1); AH = - 285.5 kJ/mol 3 C(s) + 4 H2(g) → C3H8 (g); AH r = - 103.8 kJ/mol
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7- (15 pts) Calculate the standard enthalpy of formation of CS2 (1) given that a. C(s) + O2(g) + CO2(g) b. S(s) + O2(g) → SO2(e) C. CS2() + 302(g) → CO2(g) + ' 250 (6) AH° = -393.5 kJ/mol AH° = -296.4 kJ/mol AH° = -1073.6 kj/mol (the standard state of the element Sulfur is S(s))
The combustion of lauric acid is given by the following
thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) +
12 CO2(g) Hcomb is −7377 kJ mol−1 Using the heats of formation
for CO2(g) and H2O(l) calculate the heat of formation (△fH) of
lauric acid. △fH△ CO2(g) = −393.5 kJ mol−1 fH
H2O(l)= −285.8 kJ mol−1
19. The combustion of lauric acid is given by the following thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) + 12 CO2(g) AH...
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