Calculate the standard free energy change at 25°C for the
reaction
2 NO(g) + O2(g) → 2 NO2(g).
Species ΔH°f, kJ/mol S°, J/(K ·
mol)
NO (g) 91.3 210.7
O2 (g) 0.0 205.0
NO2 (g) 33.2 240.0
A) -157.8 kJ
B) -532.6 kJ
C) -72.6 kJ
D) -4.7 kJ
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) →...
Pi T2 = P₂ T 12) Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). 12 46°E AH-TAS Species | AHºf, kJ/mol NO () 91.3 02 (8) 0.0 NO2 (8) 5, J/(K.mol) 210.7 205.0 240.0 33.2 A) -4.7 kJ (B) -72.6 kJ C) -157.8 kJ D) -532.6 kJ 13) The Boltzmann formula is S=k In W. A perfect crystal has a molar entropy of 0 at absolute zero because A) W=NA...
2- Therro dynamics e that best completes the statement or answers the question TIPLE CHOICE. Choose the one alternative that best completes the at 1) The SI unit for pressure is the A) newton. B) pascal C) MM Hg D) atmosphere. 2) The mixing of different gases by random molecular motion with freque A) diffusion. B) Dalton's law. C) compressibility. D) effusion 3) Entropy is a measure of A) the rate of a reaction. C) molecular randomness. B) free energy...
Use the table to calculate the energy change in J/K of each reaction below (assume standard thermodynamic conditions 1.00 atm and 298.15 K) Substance S (J.mol -1. K -1 Br2 (l) 152.23 HBr (g) 198.59 C (diamond) 2.38 CH4 (g) 186.2 CH3OH (l) 126.8 CO (g) 197.6 CO2 (g) 213.6 O2 (g) 205.0 H2 (g) 130.6 H2O (g) 188.7 N2 (g) 191.5 NO (g) 210.7 NH3 (g) 192.3 NO (g) 210.7 NO2 (g) 240.0 K2CO2 (s) 155.52 KOH (s) 78.91 S (rhombic) ...
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)
3) Calculate the standard free energy change (Go ) at 25 C for C (s) + O2 (g) ----- > CO2 (g) For which the value of Ho = -393.51 KJ/mol And the value for So = 2.83 J/mol K
23. Question (1 point) W Calculate the free-energy change of the following reaction at 221°C: C2H(g) +302(g) → 2002(g) + 2H20(g) A Hºt, kJ/mol 52.3 Sº, J/mol K 219.5 C2H4(g) O₂(g) CO2(g) H2O(g) -393.5 205.0 213.6 188.7 -241.8 1st attempt
Determine if the following reaction is spontaneous or not 25°C by determining the free energy value. 2 NO2(g) yields N2O4(g) ΔH= -57.2 kJ/mol ΔS = -175.9 J/ mol•
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 kJ/mol
Calculate the standard entropy change for the reaction P4(g)+5O2(g)→P4O10(s) using the data from the following table: Substance ΔH∘f (kJ/mol) ΔG∘f (kJ/mol) S∘ [J/(K⋅mol)] P4(g) 58.9 24.5 279.9 O2(g) 0 0 205.0 P4O10(s) −2984 −2698 228.9