Calculate ΔGrxn for the dissociation of N2O4 at 25°C with P(N2O4) = 0.150 bar and P(NO2) = 0.100 bar. Use the data provided below.
ΔG°f (kJ/mol)
N2O4(g) 99.8
NO2(g) 51.3
N2O4 ----> 2NO2
∆G° =( 2×51.3) - (99.8)
= 2.80 kJ/mol
Q = (0.10)2/0.150
= 0.067
∆Gr = ∆G° + RT×ln(K)
= 2.80 + 8.314×298×ln(0.067)
= -3.91 kJ/mol
Calculate ΔGrxn for the dissociation of N2O4 at 25°C with P(N2O4) = 0.150 bar and P(NO2)...
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the reaction 2 NO2(g) →N2O4(g) .(a) Using ΔGfN2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.kJ(b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.25 atm and 1.30 atm, respectively.kJ
For the dimerization of nitrogen dioxide, ΔG° = −4.7 kJ at 25°C. 2 NO2(g) ⟶ N2O4(g) Calculate ΔG for this reaction if the partial pressures of NO2 and N2O4 are both 0.38 atm. (R = 8.31 × 10−3 kJ/K) a. -10.86 kJ b. -11.36 kJ c. -15.12 kJ d. -11.07 kJ e. -7.10 kJ
Calculate K at 298 K for the following reaction given the Gibbs free energy of formations 213) substance! ΔG。 kJ/mol N2O4(g) +99.8 NO2(g)+51.3 1.13 0.32 3.1
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...
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)
calculate ΔGrxn at 36 ∘C. N2O4(g)→2NO2(g)
Calculate the equilibrium concentrations of N2O4and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0150 M and [NO2]= 0.0360 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Part A Calculate the equilibrium concentration of N2O4. Express your answer with the appropriate units. Part B Calculate the equilibrium concentration of NO2. Express your answer with the appropriate units.
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0130 M and [NO2]= 0.0300 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. I've worked through this problem a few times and still don't get the right answer. Can anyone show me the work??
Calculate the equilibrium concentrations of N2O4 and NO2 at 25°C in a vessel that contains initial concentration of 0.0500M of N2O4. KC = 4.64 × 10-3 at 25°C. N2O4 (g) 2NO2 (g)