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You have two reactions
A+B---> 2C. K1
C----> 1/2A+1/2B. K2
How are K1 and K2 related?
A.) K2=(1/K1)1/2
B.) K2=1/K1
C.) K2=K12
D.) K2=(1/2)K1
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- The equilibrium constant for the reaction2 NO1g2 + Br21g2 ∆ 2 NOBr1g2is Kc = 1.3 * 10-2 at 1000 K. (a) At this temperature doesthe equilibrium favor NO and Br2, or does it favor NOBr?(b) Calculate Kc for 2 NOBr1g2 ∆ 2 NO1g2 + Br21g2.(c) Calculate Kc for NOBr1g2 ∆ NO1g2 + 12 Br21g2.At 2452 oC, Keq = 97.7 for the reaction: 1/3 NO2(g) + 1/3 N2O(g) (equlibrium arrows) NO(g) (a) What is the value of Keq for the reaction NO(g) 1/3 NO2(g) + 1/3 N2O(g)?Keq = .(b) What is the value of Keq for the reaction NO2(g) + N2O(g) 3 NO(g)?Keq = .(c) What is the value of Keq for the reaction 3 NO(g) NO2(g) + N2O(g)?Keq = .Compound ΔHf (kj/mol) C2H5OH(i) -277.6 H2O(i) -285.8 H2O(g) -241.8 CO2(g) -393.5 CO(g) -110.5 H2O2(i) -187.6 C3H8(g) -103.8 What is the ΔH for the following reaction? C2H5OH(i) + 3O2 (g) --> 2CO2(g) + 3H2O(i)
- Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. C2H2(g) + H2(g) → C2H4(g) S°(J/mol∙K) 200.9 130.7 219.3Which of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)For which reaction below would you expect to have the largest orientation factor (p)?(a) N2(g) + 3 H2(g) → 2 NH3(g)(b) O3(g) + O(g) → 2 O2(g)(c) CH3OH(l) + HCl(g) → CH3Cl(l) + H2O(l)(d) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
- From the attached solution where did you get this? = S CO2 (g) + S H2O (l) - [ S C6H12O6 (s) + S O2(g)] = (213.7 J/mol-K + 69.9 J/mol-K) - (212.0 J/mol-K + 205.1 J/mol-K)Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) S°(J/mol • K) 192.8 205.2 210.8 188.817 Calculate the ΔH°rxn for the following reaction. SiO2(s) + 4HCl(g) → SiCl4(g) + 2H2O(g) ΔH°f [SiO2(s)] = –910.9 kJ/mol; ΔH°f [SiCl4(g)] = –657.0 kJ/mol; ΔH°f [HCl(g)] = –92.3 kJ/mol; ΔH°f [H2O(g)] = –241.8 kJ/mol Group of answer choices –139.5 kJ –137.4 kJ –104.4 kJ 104.4 kJ 139.5 kJ
- Calculate ΔG°rxn for the following reaction. The ΔG°f for each species is shown below the reaction. 4 ABO3 (g) + 5 B2A4 (l) → 7 B2 (g) + 12 A2O(l) ABO3 (g) B2A4 (l) B2 (g) A2O(l) ΔG°f (KJ/mol) -73.5 149.3 0 -237.1For the competing reactions 2A-->R with rate constant k1 and 2A-->S with rate constant k2, the concentration of R is 3 M while that of S is 0.2 M when starting with 10 M of pure A after 1 hr. a) What is the selectivity if R is the desired product? (A) 50 (C) 1/15 (B) 10/3 (D) 15 b) What is the remaining amount of A? (A) 4 M (C) 36 M (B) 18 M (D) 7.2 MThe Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the solubility of Al(OH)3 in g/L?