Use the standard reaction enthalpiesgiven below to determine AH°rxn forthe following reaction:rxn8 SO3(g) →8 S(s) + 12 O₂(g) AHᵒr= ?Given:SO₂(g) → S(s) + O₂(g) AH°rxn+296.8 kJ=2 SO₂(g) + O₂(g) → 2 SO3(g) AH rxn= -197.8 kJa. -692.4 kJb. 3166 kJc. -791.4 kJd. -3166 kJe. -494.6 kJ

Answered: Image /qna-images/answer/12da9617-d467-45fc-abd8-acecddc58ee2.jpg

Use the standard reaction enthalpies given below to determine ΔΗ, for the following reaction: rxn 8 SO3(g) →8 S(s) + 12 O₂(g) AH°rxn = ? Given: SO₂(g) →S(s) + O₂(g) AH°, +296.8 kJ = 2 SO₂(g) + O₂(g) → 2 SO3(g) AH rxn = -197.8 kJ a. -692.4 kJ b. 3166 kJ c. -791.4 kJ d. -3166 kJ e. -494.6 kJ

Use the standard reaction enthalpies given below to determine ΔΗ, for the following reaction: rxn 8 SO3(g) →8 S(s) + 12 O₂(g) AH°rxn = ? Given: SO₂(g) →S(s) + O₂(g) AH°, +296.8 kJ = 2 SO₂(g) + O₂(g) → 2 SO3(g) AH rxn = -197.8 kJ a. -692.4 kJ b. 3166 kJ c. -791.4 kJ d. -3166 kJ e. -494.6 kJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Using the equations Ca(s) + 1/2 0, (g) → CaO (s) AH° = -450 kJ/mol CO, (g) → C (s) + O, (g) AH° = 394 kJ/mol Determine the enthalpy for the reaction C(s) + 2 CaO(s) → CO, (g) + 2 Ca(s). KJ/mol 1 2 3 6. C 7 8 9. +/- х 100 4.
The hypothetical element X and an oxide of X undergo the following reactions with oxygen, with the listed enthalpy changes: 4 X(5) + 3 02(g) – 2 X203(g) AHrxn = -400.0 kJ 4 XO2(g) – 2 X203(g) + O2(g) AHrxn - +200.0 kJ Using the above information, determine AHrxn for the following reaction: X(S) + O2g) – XO22) O -200.0 k) O -600.0 kJ O -150.0 k) O 200.0 kJ
When methanol, CH, OH, is burned in the presence of oxygen gas, O,, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH, OH(g) + 0,(g) → CO,(g) + 2 H,O(1) ΔΗ --764 kJ How much methanol, in grams, must be burned to produce 837 kJ of heat?
Use the standard reaction enthalpies given below to determine ΔH°rxn for the followingreaction: P4(g) + 10 Cl2(g) → 4PCl5(s) PCl5(s) → PCl3(g) + Cl2(g) P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = ?? ΔH°rxn = +157 kJ ΔH°rxn = -1207 kJ
Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI, (aq) + 3 H, (g) ΔΗ = -550.0 kJ 2. HCl(g) HCI(aq) AH2 = -74.8 kJ > 3. H, (g) + Cl, (g) → 2 HCl(g) AH3 = -1845.0 kJ 4. MCl, (s) → MCI, (aq) AH4 = -291.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) ΔΗ kJ
Using the following thermochemical equations; (a) CaO (s) + Cl2 (g) → CaOCl2 (s) ΔH°= -110.9 kJ(b) CaO (s) + H2O (l) → Ca(OH)2 (s) ΔH°= -65.1 kJ(c) H2O (l) + CaOCl2 (s) + Br2 (l) → Ca(OH)2 (s) + Br2 (l) +2 NaCl (s) ΔH°= -60.2 kJDetermine the value of ΔH° in kJ for the following reaction:½ Cl2 (g) + NaBr (s) → ½ Br2 (l) + NaCl (s)
Methanol (CH3OH) can be used as the fuel in a "canned heat" container that is used to keep food hot on a buffet table. The combustion of methanol can be described by the following BALANCED thermochemical equation: 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) ΔH° = –1199 kJ Calculate the enthalpy change, in kilojoules, when 151.3 g of methanol is burned via this reaction?
What is the standard molar enthalpy of formation for aluminum oxide (Al203) based on the thermochemical equations provided? 4Fe(s) + 302(g) → 2FE203(s) AH° = -1648.4 kJ/mol 2Al(s) + Fe203(s) --> 2Fe(s) + Al203(s) AH° = -851.5 kJ/mol O 3351.4 kJ/mol O -796.9 kJ/mol O-2499.9 kJ/mol O -1675.7 kJ/mol
The standard enthalpy change for the following reaction is -135 kJ at 298 K. 1/2 N2(g) + 1/2 H2(g) + 3/2 O2(g) HNO3(g) ΔH° = -135 kJ What is the standard enthalpy change for the reaction at 298 K? N2(g) + H2(g) + 3 O2(g)2 HNO3(g) kJ
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9) Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9)