For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN....
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) Delta G^ =-4.78 J/mol . Calculate K at 25°C
Using the given data, determineArGº at 298 K for the precipitation reaction below. Ag+(aq) +r(aq) → AgI(5) Substance AGº(kJ/mol) at 298 K r(aq) 51.59 Ag (aq) 77.12 AgI(s) -66.2 Select one: O a. 62.5 kJ/mol-rxn O b.-40.7 kJ/mol-1xn OC. 91.7 kJ/mol-rxn O d. -91.7 kJ/mol-xn O e. 40.7 kJ/mol-rxn
15. Consider the reaction 2 NO2(g) N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and Gf NO2(g) = 51.3 kJ/mol, calculate G° at 298 K. kJ (b) Calculate G at 298 K if the partial pressures of NO2 and N2O4 are 0.35 atm and 1.60 atm, respectively. kJ 16. Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ (b) Calculate G at 298 K...
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌N2O4 (g) The conditions for this reaction are: PNO2 = 1.40 bar PN2O4 = 1.98 bar
Find ΔrG for reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌ N2O4 (g) Given Conditions: Pressure: NO2 = 1.25 bar Pressure: N2O4 = 0.65 bar N2O4(g) --
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
For a particular reaction, AH = -14.20 kJ/mol and AS = -198.5 J/(mol.K). Calculate AG for this reaction at 298 K. AG = 73.35 kJ/mol
Calculate ΔSsurr at the indicated temperature for a reaction. A) ΔH∘rxn= -294 kJ ; 298 K B) ΔH∘rxn= -294 kJ ; 78 K C) ΔH∘rxn= 145 kJ ; 298 K D) ΔH∘rxn= 145 kJ ; 78 K
Calculate ΔSsurr at the indicated temperature for a reaction: A) ΔH∘rxn= -283 kJ ; 298 K B) ΔH∘rxn= -283 kJ ; 72 K C) ΔH∘rxn= 140 kJ ; 298 K D) ΔH∘rxn= 140 kJ ; 72 K