As the value of K remains same for consecutive experiment therefore it is clear that reaction follows first order kinetics.
a) Calculate K at 298 K for the following reaction: NO(g) + 1 2 O2(g) ? NO2(g) ?G0f(kj/mol) NO(g) 86.60 NO2(g) 51 O2(g) 0 K = ×10
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Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
What is ∆So at 298 K for the following reaction? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH°f (kJ/mol) -20.6 -296.8 -241.8 Δ G°f( kJ/mol) -33 -300.2 -228.60
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all speies. For the reactionC2H6(g)+H2(g)↽−−⇀2CH4(g)the standard change in Gibbs free energy is Δ𝐺∘=−32.8 kJ/mol.ΔG°=−32.8 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are 𝑃C2H6=0.400 bar,𝑃H2=0.150 bar, and 𝑃CH4=0.850 bar?𝑃CH4=0.850 bar? Δ𝐺=_____ kJ/molSk
03(g) + OH(g) =H(g) + 2 O2(g) AG° = 5.8 kJ/mol at 298 K, A,Gº = 0 kJ/mol at 354 K, and 4 Gº = -2.0 kJ/mol at 373 K. (a) Calculate the equilibrium constant value for this reaction at 298K, 354 K, and 373 K. (b) At 354K, calculate the change in the Gibbs energy of the reaction, AG when the partial pressures of O3 and OH are kept at 10 bar and 30 bar, respectively, while O2 and...
(3 Points) Calculate the standard Gibbs energy of reaction for the reaction below at 298 K and 596 K. 4 HCl(g) + O2(g) 2Cl2(g) + 2H2O(l) Assume that the heat capacities are constant over the temperature range involved. 02(g) Cl2(g) HCl(g) 4,Hº (kJ mol-4) -92.11 S JK- mol-) 186.91 Comº (K-mol-4) 29.12 AG° (k mol-1) | -95.30 223.07 205.14 9.36 H2O(1) -285.83 69.91 75.29 -237.133 2 33.91
1--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? CH4 (g) + 2 O2 (g) ⇌ CO2 (g) + 2 H2O (g) The conditions for this reaction are: PCH4 = 0.73 bar PO2 = 0.27 bar PCO2 = 0.10 bar PH2O = 1.41 bar 2--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 =...
The decomposition of N2O5 proceeds according to the following equation 2 N2O5(g) → 4 NO2(g) + O2(g). The rate constant, k, for the reaction at 298 K is 2.20 x 10-3 min-1. If a reaction is set up in a vessel at 298 K, with an initial concentration of 0.278 mol L-1; what is the concentration of reactant N2O5(g) in mol/L after 40.2 minutes? Report your answer without units
What is the ΔS° at 298 K for the following reaction? 2 O3(G) ---- 3 O2(G) Substance ΔS° (J/mol·K) O2(g) 205.0 O3(g) 238.8