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- Consider the reaction below: 2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g) A sealed reactor contains a mixture of SO₃(g), SO₂(g), and O₂(g) with partial pressures: 0.200 bar, 0.250 bar and 0.300 bar, respectively. Calculate Kp if the O₂(g) partial pressure is 0.275 bar when the mixture achieves equilibrium..Find ∆H as a function of T for the reaction: CO2 (g) + C (s, graphite) = CO Given that ∆H 293= 41,400 cal Cp CO2= 5.166+15.77×10^-3 T - 95.78×10^-3 T² + 2.260×10^-9 T³ Cp CO= 6.6 + 2×10^-3 T Cp C (s, graphite)= 2.673 + 2.617×10^-3 T - 1.169×10^-5 T^-2For the reaction S(s,rhombic) + 2co(g)----> so2(g) +2c(s, graphite) Delta H =75kj and delta s= -167.6j/k The equilibrium constant for this reaction at 298.0 k is ----- Assume that delta h and delta s are independent of temperature.
- The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.The following questions refer to the following reaction at constant 25°C and 1 atm.2Fe(s) + (3/2)O2(g) + 3H2O(l) 2Fe(OH)3(s) H = –789 kJ/molSubstance S° (J/mol K)Fe(OH)3(s) 107Fe(s) 27O2(g) 205H2O(l) 70a. Determine Ssurr for the reaction (in kJ/mol K)b. Determine Suniv for the reaction (in kJ/mol K)2.65c. What is the G for this reaction?d. Calculate the equilibrium constantCO(g)+2H2(g)⇌CH3OH(g) K = 2.18×102 at 340 K Calculate ΔrG for the reaction at 340 K in STANDARD CONDITIONS please Express your answer using three significant figures and include the appropriate units.
- For the reaction C(s) + CO2 (g) -> 2CO (g) determine kp and kc at 1000K and at 1100k4 One mole of N2O4 is introduced into a constant pressure chamber at a temperature of 298.15 K and a pressure of 0.1 bar. Calculate the fraction of dissociation (α) of N2O4 [to 2NO2 (g)] when the reaction reaches equilibrium under these conditions. Calculate ΔGrxn for the reaction at values of the extent of reaction α of 0.1, 0.4, 0.6, and 0.9 moles. (Note -- the reaction is not at equilibrium at these extents of reaction.)Consider this reaction: CO(g)+2H2(g)⇌CH3OH(g) )K=2.18×102 at 340 K Calculate ΔrG for the reaction at 340 K under each of the following conditions: A) Standard conditions B) Equilibrium C) PCO = PH2 = 0.0010 bar, PCH3OH = 1.0 bar
- 13) Consider the reaction N2O (g) + NO2 (g) -----> 3NO (g) k= 4.4 x 10-19 a) calculate the Delta G0 at 25C for the reaction b) calculate Delta Gf0 for N2O Delta Gf0 for NO2 (g) and NO (g) are 51.3 and 86.6 Kj/mol at 25C, respectivlyIn the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species, kx, kp and ∆G0The following reaction was carried out in a 4.00 LL reaction vessel at 1100 KK: C(s)+H2O(g)⇌CO(g)+H2(g)C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 5.00 molmol of CC, 12.1 molmol of H2OH2O, 3.20 molmol of COCO, and 6.50 molmol of H2H2, what is the reaction quotient Qc�c? Enter the reaction quotient numerically.