For the reaction N2O3(g) NO(g)+NO2(g) Delta G^ =-4.78 J/mol . Calculate K at 25°C
For the reaction N2O3(g) → NO(g) + NO2(g) ΔG° = -4.78 J/mol. Calculate K at 25°C. A. 1.023 B. 1.002 C. 1.010 D. 0.9484
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN. Compute K for this reaction. a) 1.01 Ob) 0.998 O c) 0.948 O d) 6.89 Oe) 10.23
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
The rate of decomposition of N2O3(g)N2O3(g) to NO2(g)NO2(g) and NO(g)NO(g) is followed by measuring [NO2][NO2] at different times. The following data are obtained. [NO2](mol/L)[NO2](mol/L) 0 0.193 0.316 0.427 0.784 t(s)t(s) 0 884 1610 2460 50,000
For the reaction: 2C4H10(g)+13O2(g)-->8CO2(g)+10H20(g) delta H is -125kJ/mol and delta S is 253 J/K*mol. This reaction is_. a) spontaneous at all temperatures b) spontaneous only at high temperatures c) spontaneous only at low temperatures *I know the answer is A, but I need a detailed explanation as to why that is the correct answer.
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 Kp at 298 K for the reaction SO.(g) + NO2()SO3(g)+NO() SO2(g) SO3(g) NO(g) NO2(g) -300.4 k/mol -370.4 kJ/mol 86.7 kJ/mol 51.8 kJ/mol For the reaction 2NO(g)+02(g)- 2NO2( f iniially P(NO)1.5 atm, PO2)-1.4 atm, and P(NOJ-2.0 atrn, calculate Δ@for this reaction at 25°C. The following data is valid at 25°C: NO NO2 AGe(kJ/mol 86.7 51.8
Calculate ΔS∘rxn for the reaction 2NO(g)+O2(g)→2NO2(g) Substance S∘ (J/mol⋅K) NO2 240.0 O2 205.2 NO 210.8
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...
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is the reaction spontaneous at room temperature? If no, at what temperature (in K and C) does this reaction become spontaneous?