Yq0o20 qa oldialv-feloivatil Amax for the transition in ethylene is 170 nm. Is the HOMO-LUMO energy difference in ethylene greater than or less than that of cis, trans-1,3-cyclooctadiene (230 nm)? Problem 14.25
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- Q26 (D) Explain with figure the role of a catalyst on speed of areaction.Calculate the ΔS°rxn of the following reaction at 215°C and standard pressure. C2H4 (g)+302 (g)->2CO2 (g)+2H2 ΔHºf, kJ/mol Sº, J/mol•K ΔGºf, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 0 205.0 0 CO2(g) -393.5 213.6 -394.4 H2O(g) -241.8 188.7 -228.6 _____ J/mol*KFrom the data given below calculate the value of ΔS° for the reaction. T = 298.15 K. A(g) + 1B(g) ---> 1C(s) + D(l)ΔfH°/(kJ mol-1) -393.23 -44.71 -332.49 -284.45ΔfG°/(kJ mol-1) -392.07 -15.56 -197.3 -231.43
- Predict the general tempature and pressure conditions for the optimum conversion of ethylene (C2H4) to ethane (C2H6).True or False: 1. The initial concentration of an intermediate is assumed as 0 when using steady-state approximation. 2. A spontaneous reaction with ΔG = -1070 J/mol happens at 562 K, the Keq of this process is less than 1.The Ea for the uncatalyzed reaction of 5-Carboxyuracil decarboxylation is 1.2 x105 J/moland the frequency factor (pre-exponent A) is 1.6 x 1012 s-1. Using these values what isthe rate constant for this reaction at 340K?
- The value of ΔS° for the catalytic hydrogenation of acetylene to ethene, C2H2 (g) + H2 (g) → C2H4 (g) is __________ J/K∙ mol. Substance S (J/K-mol) C2H2 200.8 H2 130.6 C2H4 219.4 a. -112.0 b. 550.8 c. -18.6 d. 112.0 e. 18.6What would be the state order for the following reaction: 2H2+O2-----2H2O A. Zero b. First c. Second d. You cannot predict based on the given informationWrite the expression for Kc for the following reactions. Ineach case indicate whether the reaction is homogeneousor heterogeneous.(a) 3 NO1g2 ∆ N2O1g2 + NO21g2(b) CH41g2 + 2 H2S1g2 ∆ CS21g2 + 4 H21g2(c) Ni1CO241g2 ∆ Ni1s2 + 4 CO1g2(d) HF1aq2 ∆ H+1aq2 + F-1aq2(e) 2 Ag1s2 + Zn2+1aq2 ∆ 2 Ag+1aq2 + Zn1s2(f) H2O1l2 ∆ H+1aq2 + OH-1aq2(g) 2 H2O1l2 ∆ 2 H+1aq2 + 2 OH-1aq2
- For the reaction 2C(s) + H2(q) -> C2H2 Calculate ΔH use a diagram and data below. ΔHcc2H2 =-1299.6KJ ΔHcc = -393.5KJ ΔHcH2 =-285.8KJ ΔH= 2x(-393.5) + (-285.8) + (-1299.6) = -512.6 – 285.8 = 798.4Consider the following mechanism: 1) Br2(g) = 2Br(g) Kc1 = 2.2 x 10^-3 2) Br(g) + H2(g) = HBr(g) + H(g) Kc2 = 7.5 x 10^6 3) H(g) + Br(g) = HBr(g) Kc3 = 350 calculate Kc for the overall reactionConsider the following ∆H°f and S° at 300K: Chemical species ∆H°f S° (in J/mol. K) C2H6(g) -83.7 229.6 H2O(g) -241.82 188.83 CO2(g) -110.53 199.42 O2(g) 0 205.138 A) Determine the ∆H°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) B) Determine the ∆S°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) C) Determine the ∆G°rnx of the following reaction at 300K (in kJ/mol) C2H6(g) + 7/2 O2(g) → 3 H2O (g) + 2 CO2(g) Show the process and calculations