Using values from Appendix C in the textbook, calculate the standard enthalpy change for each of the following reactions.
Link to Appendix C: https://media.pearsoncmg.com/ph/esm/esm_brown_chemistry_14/appendices/appendix-c.pdf
1. 2SO2(g)+O2(g)→2SO3(g)
2. Mg(OH)2(s)→MgO(s)+H2O(l)
3. N2O4(g)+4H2(g)→N2(g)+4H2O(g)N2O4(g)+4H2(g)→N2(g)+4H2O(g)
4. SiCl4(l)+2H2O(l)→SiO2(s)+4HCl(g)
(1.) Balanced equation : 2 SO2 (g) + O2 (g) 2 SO3 (g)
Standard enthalpy change, Ho = Hof products - Hof reactants
Ho = 2 * Hof SO3 (g) - [2 * Hof SO2 (g) + Hof O2 (g)]
Ho = 2 * (-395.2 kJ/mol) - [2 * (-296.9 kJ/mol) + (0)]
Ho = -790.4 kJ + 593.8 kJ
Ho = -196.6 kJ
(2.) Balanced equation : Mg(OH)2 (s) MgO (s) + H2O (l)
Standard enthalpy change, Ho = Hof products - Hof reactants
Ho = [Hof MgO (s) + Hof H2O (l)] - Hof Mg(OH)2 (s)
Ho = [(-601.8 kJ/mol) + (-285.83 kJ/mol)] - (-924.7 kJ/mol)
Ho = -887.63 kJ + 924.7 kJ
Ho = 37.07 kJ
(3.) Balanced equation : N2O4(g) + 4 H2(g) N2(g) + 4 H2O(g)
Standard enthalpy change, Ho = Hof products - Hof reactants
Ho = [Hof N2(g) + 4 * Hof H2O(g)] - [Hof N2O4(g) + 4 * Hof H2(g)]
Ho = [(0) + 4 * (-241.82 kJ/mol)] - [9.66 kJ/mol + 4 * (0)]
Ho = -967.28 kJ - 9.66 kJ
Ho = -976.94 kJ
Q4. Balanced equation : SiCl4(l) + 2 H2O(l) SiO2(s) + 4 HCl(g)
Standard enthalpy change, Ho = Hof products - Hof reactants
Ho = [Hof SiO2(s) + 4 * Hof HCl(g)] - [Hof SiCl4(l) + 2 * Hof H2O(l)]
Ho = [(-910.9 kJ/mol) + 4 * (-92.30 kJ/mol)] - [(-640.1 kJ/mol) + 2 * (-285.83 kJ/mol)]
Ho = -1280.1 kJ + 1211.76 kJ
Ho = -68.34 kJ
Using values from Appendix C in the textbook, calculate the standard enthalpy change for each of...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
Use data given below to calculate ΔrS∘ΔrS∘ for each of the reactions. Standard Thermodynamic Quantities for Selected Substances at 25 ∘C∘C Substance ΔrS∘ΔrS∘, JK−1mol−1JK−1mol−1 Cr(s)Cr(s) 23.8 Cr2O3Cr2O3(s)(s) 81.2 CO(g)CO(g) 197.7 CO2(g)CO2(g) 213.8 H2(g)H2(g) 130.7 H2O(g)H2O(g) 188.8 H2O(l)H2O(l) 70.0 HNO3(aq)HNO3(aq) 146.0 N2(g)N2(g) 191.6 N2O4(g)N2O4(g) 304.4 NO(g)NO(g) 210.8 NO2(g)NO2(g) 240.1 O2(g)O2(g) 205.2 SO2(g)SO2(g) 248.2 SO3(g)SO3(g) 256.8 A) 4NO2(g)+2H2O(l)+O2(g)→4HNO3(aq) B) Cr2O3Cr2O3(s)(s) +3CO(g)→2Cr(s)+3CO2(g) C) SO2(g)SO2(g) +12O2(g)→SO3(g) D) N2O4(g)+4H2(g)→N2(g)+4H2O(g)
calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ
Using Thermodynamic Data (∆Hf), calculate the enthalpy change (∆Hrxn) for the following reactions: Fe2O3 (s) + H2 (g) → Fe (s) + H2O (l) N2H3CH3 (l) + N2O4 (l) → H2O (g) + N2 (g) + CO2 (g) C6H12O6 (s) + O2 (g) → CO2 (g) + H2O (g)
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: (a) 4 NH3(g) + O2(g) 2 N2H4(g) + 2 H2O(l) Keq = . (b) CH4(g) + 4 Cl2(g) CCl4(l) + 4 HCl(g) Keq = . (c) 6 C(graphite) + 6 H2O(l) C6H12O6(s) Keq = .
Using data from Appendix C in the textbook, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K . A) NaHCO3(s) ⇌ NaOH(s)+CO2(g) What is the free-energy change for this reaction at 298 K? Express the free energy in kilojoules to one decimal place. B) 2HBr(g)+Cl2(g) ⇌ 2HCl(g)+Br2(g) Which is the equilibrium-constant expression for this reaction? K=P2HClPBr2P2HBrPCl2 K=P2HBrPCl2 K=P2HBrPCl2P2HClPBr2 K=PHClPBr2PHBrPCl2 C) 2SO2(g)+O2(g) ⇌ 2SO3(g) Which is the equilibrium-constant...
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: Using values from Appendix C of your textbook, calculate the value of Keg at 298 K for each of the following reactions: (a) Fe3O4(s) + 4 CO(g) = 3 Fe(s) + 4 CO2(g) Keq = (b) Fe2O3(s) + 6 HCI(g) = 2 FeCl3(s) + 3 H2O(g) Keq = D . (c) 4 NH3(g) + O2(g) = 2 N2H4(9)...
problem 5.72 please assist with parts a,b,c and d. Using values from Appendix C or the internet calculate the value of ΔH∘ for each of the following reactions. a. 4HBr(g)+O2(g)→2H2O(l)+2Br2(l) express answer using five sig figs ΔH∘rxn =...............kJ b. 2NaOH(s)+SO3(g)→Na2SO4(s)+H2O(g)2NaOH(s)+SO3(g)→Na2SO4(s)+H2O(g) (ΔHf∘ Na2SO4Na2SO4 = -1387.1 kJ/molkJ/mol) ΔH∘rxn =...........kJ answer using four sig figs c. CH4(g)+4Cl2(g)→CCl4(l)+4HCl(g) ΔH∘rxn..............kJ express answer in four sig figs d. Fe2O3(s)+6HCl(g)→2FeCl3(s)+3H2O(g) ΔH∘rxn..............kJ express answer in two sig figs
12) Use the following data to calculate the standard heat (enthalpy) of formation, ???, of manganese(IV) oxide, MnO2 (s). 2MnO2(s)--2MnO(s) + O2(g) MnO2(s) + Mn(s)- 2Mn0(s) ??-264 kJ ?? -240 kJ 13) Calculate the ??0nn for the following reaction. (Arf [SiO2(s)--910.9 kJ/mol; APf [SiCl4(g)]--657.0 kJ/mol; ??'f [HCI(g)1--92.3 kJ/mol; ? Hof [H2O(g),- -241.8 kJ/mol) SiO2(s) + 4HCI(g)-SiCI(g) + 2H2O(g)
Calculate the standard enthalpy of reaction for the following reaction using the appropriate standard enthalpies of formation ΔH°f [SiCl4 (g)] = -657.0 kJ/mol SiO2 (s) + 4 HCl (g) → SiCl4 (g) + 2 H2O (g)