21.) Calculate the enthalpy of hydrogenation of benzene to cyclohexane from the followingreactionsA,H (kJ/mol)C6H6 (1) + 15/2 02 (g) → 6 CO2 (g) + 3 H20 (1)C6H12 (1) + 9 02 (g) → 6 CO2 (g) + 6 H20 (1)H2 (g) + ½ 02 (g) → H2O (1)-3268-3920-285.83a.) -205 kJ/molb.) -1507 kJ/molc.) -938 kJ/mold.) -366 kJ/mol

The reactions given are, 1) C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) ΔH…

21.) Calculate the enthalpy of hydrogenation of benzene to cyclohexane from the following reactions A,H (k)/mol) -3268 COH6 (1) + 15/2 Oz (g) → 6 CO2 (g) + 3 H20 (I) C&H12 (1) + 9 02 (g) → 6 CO2 (g) + 6 H2O (1) H2 (g) + ½ O2 (g) -3920 -285.83 H2O (1I) a.) -205 kJ/mol b.) -1507 kJ/mol c.) -938 kJ/mol d.) -366 kJ/mol

21.) Calculate the enthalpy of hydrogenation of benzene to cyclohexane from the following reactions A,H (k)/mol) -3268 COH6 (1) + 15/2 Oz (g) → 6 CO2 (g) + 3 H20 (I) C&H12 (1) + 9 02 (g) → 6 CO2 (g) + 6 H2O (1) H2 (g) + ½ O2 (g) -3920 -285.83 H2O (1I) a.) -205 kJ/mol b.) -1507 kJ/mol c.) -938 kJ/mol d.) -366 kJ/mol

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.50QE

See similar textbooks

Similar questions

Using a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.
Calculate the enthalpy of combustion for kerosene. Assume that kerosene is C10H22(l) and that the products are CO2(g) and H2O(l). ΔH°f (C10H22(l)) = –249.6 kJ/mol ΔH°f (CO2(g)) = –393.5 kJ/mol ΔH°f (H2O(l)) = –285.8 kJ/mol Select one: a. –872.9 kJ/mol b. –5489.9 kJ/mol c. –429.7 kJ/mol d. –6829.2 kJ/mol
(a) Calculate the standard enthalpy change for the combustion of 1 mol of benzene, C6H6(l), to CO2(g) and H2O(l).(b) Compare the quantity of heat produced by combustion of 1.00 g propane with that produced by 1.00 g benzene.
For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. C8H18 (g) + -25 0₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) AH; = ΔΗ What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? 18 -208.5 Incorrect ▲Hixn = -5108.7 kJ/mol kJ/mol
calculate (d) the molar enthalpy of combustion (AHcomb; in kJ/mol) of benzoic acid. I just need to understand how to calculate part d) the molar enthalpy of benzoic acid.
Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + H₂(g) → C₂H₂ (9) AH° = 226.7 kJ (2) 2C(s) + 2H₂(g) → C₂H₁ (9) ΔΗ° = 52.3 kJ What is the standard enthalpy change for the following reaction? (3) C₂H₂(g) + H2 (9) → C2H4 (9) AH° =? Standard enthalpy change = kJ
4 CH3NO2 (I) + 3 02(g) -> 4 CO2(g) + 6 H20(g) + 2 N2(g) [ CH = - 14.18.4] Calculate the molar enthalpy of combustion for nitromethane
From the enthalpies of the reaction H2(g)+F2(g)→2HF(g)AH=-537kJ C(s)+2F2(g) →CF4(g)AH=-680kJ 2C(s)+2H2(g) →C2H4(g)AH=+52.3kJ calculate AH for the reaction of ethylene with F2: C2H4(g)+6F2(g)→2CF4(g)+4HF(g)
powo 72 3. Calculate the heat of combustion (kJ) of propane, C3H8 using the listed standard enthalpy of reaction data: C3H8(g) + 5 O2(g) →3 CO2(g) + 4 H₂O(g) AH° = -103.8 kJ AH = -393.5 kJ AHO = -241.8 kJ 3 C(s) + 4 H₂(g) →→ C3H8(g) C(s) + O2(g) → CO2(g) H₂(g) + 1/2 O2(g) → H₂O(g) 4. Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N₂(g) + 5 O₂(g) →2 N₂O5(g) AHO=-571.6 kJ AH°= -73.7 kJ AH°=-348.2 kJ (24 2 H₂(g) + O2(g) → 2 H₂O(1) N₂Os(g) + H₂O(1)→ 2 HNO3(1) N2(g) + 3 O2(g) + H₂(g) → 2 HNO3(1) HA
Calculate the standard enthalpy change of the following hydrogenation reation of ethylene (C2H2) C2H2(g) + H2(g) → C2H4(g) Using the following information at standard conditions: 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) ∆H° = - 2600 kJ 2 C2H4(g) + 6 O2(g) → 4 CO2(g) + 4 H2O(l) ∆H° = - 2822 kJ 2 H2(g) + O2(g) → 2 H2O(l) ∆H° = - 572 kJ
Which combination will give you the enthalpy change for the hydrogenation of ethene to ethane, AH3? ΔΗ ΔΗ, 20 (s) + 3H, (g) C,H, (g) + H¿ (g) C,H, (g) AH, ΔΗ + 20,(g) + 20, (g) 200, (g) + 3H, (g) -ΔΗ +ΔΗ-ΔΗ B. ΔΗ-ΔΗ+ ΔΗ C. ΔΗ + ΔΗ-ΔΗ D. -ΔΗ-ΔΗ+ ΔΗ А.
Given the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)