a) use the data given below and calculate the deltaH, delta S , delta G and Kp at 25degrees celcius for the reaction 2NO(g) + O2 = 2 NO2(g)
b) calculate the delta G for the reaction at 250 degrees celcius
c) at what tempurature (degrees celcuis) is delta G equal to zero ? In what temperature range is this reaction product favoured?
Compound NO - Delta Hf,kJ/mol =90.9 Delta S,J/mol.K =210.76
Compount O2 - Delta Hf,kJ/mol =0 Delta S,/j/mol.K=205.14
Compound NO2 - Delta Hf,kj/mol = 33.18 Delta S,J/mol.K=240.06
a) use the data given below and calculate the deltaH, delta S , delta G and...
3. (a) Use the data given below and calculate ∆Ho, ∆So, ∆Go, and Kp at 25° C for the reaction: 4 NO (g) → 2 N2O (g) + O2 (g) (b) Calculate ∆G for the reaction at 250 °C. (c) At what temperature (°C) is ∆G equal to zero? In what temperature range is this reaction product favored? Compound ∆ Ho , kJ/mol S o , J/mol• K NO (g) 90.9 210.76 N2O (g) 82.05 219.85 O2 (g) 0 205.14
calculate the deltaH given that NO2 is 33.9 kJ mol^-1 For the reaction, 7. = -114.14 kJ mol 2NO(g) + O2(g) -> 2NO2(g), AH Calculate AH of gaseous nitrogen that AH of NO2(g) is 33.9 kJ mol. monoxide, given
Use deltaH and S to calculate DeltaG rxn... Use Delta H degree_f and S degree to calculate Delta G degree rxn (Delta G degree sys) at 25 C for the reaction below: 4 KClO3 (s) rightarrow 3 KClO4 (s) + KCl (s) Delta H degree_f KClO3 = -397.7 kJ/mol; KClO4 = -432.8 kJ/mol; KCl = -436.7 kJ/mol S degree KClO3 = 143.1 kJ/mol; KClO4 = 151.0 kJ/mol; KCl = 82.6 kJ/mol
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298 K. N2O4(g)N2O4(g) NO2(g)NO2(g) S0S0 (J/K/mol) 304.29 240.06 ΔfH0ΔfH0 (kJ/mol) 9.16 33.18 Select one or more: A. Kp=9.23Kp=9.23 , Kc=12.3Kc=12.3 B. Kp=0.563Kp=0.563 , Kc=0.33Kc=0.33 C. Kp=0.144Kp=0.144 , Kc=0.0058Kc=0.0058 D. Kp=0.355Kp=0.355 , Kc=1.23
calculate delta H for the reaction 4Cu(s)+O2(g)=2Cu2O(s) given the following hypothetical data 2Cu(s)+O2(g)=2CuO(s) delta H=-312 kJ 2Cu2OtO2(g)=4CuO(s) delta H=-340kJ deltaH=
Use the following data and the van't Hoff equation lnK2K1=ΔH∘R(1T1−1T2) to estimate a value of KP at 100 ∘C for the reaction. 2NO(g)+O2(g)⇌2NO2(g) [Hint: First determine K at 25∘C. What is ΔrH∘ for the reaction?] ΔfG∘[NO2(g)] = 51.31 kJ/mol ΔfG∘[NO(g)] = 86.55 kJ/mol ΔfG∘[O2(g)] =0 ΔfH∘[NO2(g)] = 33.18 kJ/mol ΔfH∘[NO(g)] = 90.25 kJ/mol ΔfH∘[O2(g)] =0
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
calculate delta H for the reaction C(diamond)=C(graphite) given the following data C(diamond)+O2(g)=CO2(g) deltaH=-395.45kJ C(graphite)+O2(g)=CO2(g) delta H= 393.5kJ deltaH=
Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2 (g) -> 2NO2 (g), ΔHrxn = -114.1 kJ/mol 4NO2(g) + O2 (g) -> 2N2O5 (g), ΔHrxn = -110.2 kJ/mol N2 (g) + O2 (g) -> 2 NO (g), ΔHrxn = +180.5 kJ/mol
DeltaH degree is +23 kJ mol^-1 of phosphine (PH_3) for the reaction Calculate Delta S degree for this reaction. Explain how this information allows you to determine the spontaneity or non-spontaneity of this reaction at any temperature. (S degree for PH_3 is 210 J K^-1 mol^-1.) Do these results indicate anything about the possibility of the existence of phosphine? Explain your answer.