Use data from Appendix IIB in the textbook to calculate ΔrS∘ for each of the following reactions.
CO(g)+2H2(g)→CH3OH(g)
Express your answer using four significant figures.
|
ΔrS∘ = |
JK−1mol−1
CO(g) + 2H2 (g) --------> CH3OH(g)
∆rS0 = S0( Products) - S0 ( reactant)
S0 ( Product ) = S0( CH3OH) - (( S0(H2) +S0(CO))
= (239.9- ( 2×130.59 + 197.91)) J /K mol
= -219.19 J/ K mole
Use data from Appendix IIB in the textbook to calculate ΔrS∘ for each of the following...
Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25∘C for each of the following reactions.2NO(g)+O2(g)⇌2NO2(g) Express your answer using two significant figures.
Use the data in Appendix B in the textbook to calculate ΔH∘ and ΔS∘ for each of the following reactions. From the values of ΔH∘ and ΔS∘, calculate ΔG∘ at 25 ∘C and predict whether each reaction is spontaneous under standard-state conditions. Part A 2SO2(g)+O2(g)→2SO3(g) Express your answer using four significant figures. ΔH∘ = kJ Part B Express your answer using four significant figures. ΔS∘ = J/K Part C Express your answer using four significant figures. ΔG∘ = kJ Part...
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)
2Ca(s)+O2(g)→2CaO(s) ΔrH∘= -1269.8 kJmol−1; ΔrS∘= -364.6 JK−1mol−1 Calculate the Gibbs energy change for the reaction at 24 ∘C. Express your answer using four significant figures. 2Ca(s) + O2 (g) → 2CaO(s) Δ,Ho =-1269.8 kJ mol 1: Δ,S":-3646 J K 1 mol 1 Part A Calculate the Gibbs energy change for the reaction at 24 °C. Express your answer using four significant figures. kJ mol 1 Submit Previous Answers Request Answer
Use ΔG∘f values from Appendix IIB to calculate the equilibrium constants at 25 ∘C for each of the following reactions. Br2(g)+Cl2(g)⇌2BrCl(g) ΔG∘f for BrCl(g) is -1.0 kJ/mol
70. Use data from Appendix IIB to calculate the equilibrium is constants at 25°C for each reaction. -1.0 kJ/mol. a, 2 NO2(g)一一N204(g) b. Br2(g) + Cl2(g)--2 BrCl(g) for BrCl(g)
Problem 5.74 Using values from Appendix C, calculate the value of AH for each of the following reactions. Part A Express your answer using four significant figures. AH, My Answers Give Up Part B 4Feo(s) O2 (g)-+2Fenos (s) Express your answer using four significant figures. AH, My Answers Part C Express your answer using three significant figures. AH, My Answers ue Part D
Using values of Kb in Appendix C in the textbook, calculate values of Ka for each of the following ions: Part A Propylammonium ion, C3H7NH3+ Express your answer using two significant figures. Part B Hydroxylammonium ion, NH3OH+ Express your answer using two significant figures. Part C Anilinium ion, C6H5NH3+ Express your answer using two significant figures. Part D Pyridinium ion, C5H5NH+ Express your answer using two significant figures.
Please Show Formula and Steps Using data from Appendix D in the textbook, calculate [OH?] and pH for each of the following solutions. Part A 7.0×10?2 M NaBrO. Express your answer using two significant figures. [OH?] = M SubmitRequest Answer Part B Express your answer using two decimal places. pH = SubmitRequest Answer Part C 8.3×10?2 M NaHS. Express your answer using two significant figures. [OH?] = M SubmitRequest Answer Part D Express your answer using two decimal places. pH...