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
Use ΔG∘f values from Appendix IIB to calculate the equilibrium constants at 25 ∘C for each of the...
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)
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.
Estimate the value of the equilibrium constant at 630 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K. Br2(g)+Cl2(g)⇌2BrCl(g) .ΔH∘f for BrCl(g) is 14.6 kJ/mol.
Estimate the value of the equilibrium constant at 625 K for each of the following reactions. ΔG∘f for BrCl(g) is −1.0 kJ/mol. The standard molar entropy, S∘, for BrCl(g) is 240.0 J/mol⋅K 1- 2NO2(g)⇌N2O4(g). ΔH∘f for N2O4(g) is 9.16 kJ/mol. 2- Br2(g)+Cl2(g)⇌2BrCl(g) .ΔH∘f for BrCl(g) is 14.6 kJ/mol.
Estimate the value of the equilibrium constant at 610 KK for each of the following reactions. ΔG∘fΔGf∘ for BrCl(g)BrCl(g) is −−1.0 kJ/molkJ/mol. The standard molar entropy, S∘S∘, for BrCl(g)BrCl(g) is 240.0 J/mol⋅KJ/mol⋅K. Part A 2NO2(g)⇌N2O4(g).2NO2(g)⇌N2O4(g). ΔH∘fΔHf∘ for N2O4(g)N2O4(g) is 9.16 kJ/molkJ/mol. Express your answer using three significant figures. K= ??? Part B Br2(g)+Cl2(g)⇌2BrCl(g).Br2(g)+Cl2(g)⇌2BrCl(g). ΔH∘fΔHf∘ for BrCl(g)BrCl(g) is 14.6 kJ/molkJ/mol. Express your answer using three significant figures. K= ???
Estimate the value of the equilibrium constant at 635 K for each of the following reactions. ?G?f for BrCl(g) is ?1.0 kJ/mol. The standard molar entropy, S?, for BrCl(g) is 240.0 J/mol?K. 2NO2(g)?N2O4(g). ?H?f for N2O4(g) is 9.16 kJ/mol. Br2(g)+Cl2(g)?2BrCl(g) .?H?f for BrCl(g) is 14.6 kJ/mol.
Use data from the table below to calculate the equilibrium constants at 25∘C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25∘C Substance ΔH∘f(kJ/mol) ΔG∘f(kJ/mol) S∘(J/mol⋅K) H2(g) 0 0 130.7 N2(g) 0 0 191.6 O2(g) 0 0 205.2 NO(g) 91.3 87.6 210.8 NO2(g) 33.2 51.3 240.1 CO(g) -110.5 -137.2 197.7 CO2(g) -393.5 -394.4 213.8 H2S(g) -20.6 -33.4 205.8 S2(g) 128.6 79.7 228.2 1. N2(g)+O2(g)⇌2NO(g)
Use data from the table below to calculate the equilibrium constants at 25 ?C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25?C Substance ?H?f(kJ/mol) ?G?f(kJ/mol) S?(J/mol?K) ?G of PH3=13.5, ?G of H2=0, ?G of P4=24.4 3/2H2(g)+1/4P4(g)?PH3(g)
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
For the reaction given below, the value of the equilibrium constant at 400K is 7.0 Br2(g) + Cl2(g) ßà 2BrCl(g) At equilibrium the concentration of Br2 and Cl2 are each 1 mol/L. What is the equilibrium concentration of BrCl? a. 49 mol/L b. 1.0 mol/L c. 7.0 mol/L d. 2.6 mol/L