use the information in the pK table below to determine which side of the equilibrium is favored for each of the reactions in the second table.acidPKacidpKNH₁₂36CH₁₂-C=CHNH336CHÍNH.2515.9OH10.8CH,SH10.3он10.0ii9-2CH3онSH₂-6.8OHOH-6.1CH,SH₂-7iiCH,SH2 ++Equilibrium EquationCHÍNH,CHÍNH+en.,--nCH3iiCH,SH +онCH3NH₁₂+ CH3NHii+-OH +OHLeftRightFavoredEqualFavored

Step 1: Step 2: Step 3: reaction favour in the direction from strong acid to weak acid Low pKa value…

Answered: use the information in the pK table…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section18.6: Gibbs Free Energy

Problem 2RC

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xxxvii
Consider the following equilibrium: N2O4(2) At equilibrium, the [N2O4] is equal to 2NO2 Keq = 0.133 А. 0.133 В. [NO2] [NO:] 0.133 С. 0.133 D. [NO:] [NO:] 0.133 A В O c O D
What is the direction of the equilibrium? G A B Starting materials are favoured 50:50 mixture Products are favoured POH PLOH + D
7
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.
Given each value, determine whether the starting material or product is favored at equilibrium. a.Keq = 0.5 b.ΔGo = −100 kJ/mol c.ΔHo = 8.0 kJ/mol d.Keq = 16 e. ΔGo = 2.0 kJ/mol f.ΔHo = 200 kJ/mol g. ΔSo = 8 J/(K•mol) h.ΔSo = −8 J/(K•mol)
Write the basic equilibrium equation for C,H,NH, 3. O4- D2. O+ n2+ O3+ O4+ 1 2 3 4 7 8 1 3 4 5 O6 (s) (1) (g) (aq) + -> H C OH Reset • a H,O Delete 80 888 F3 F4 F5 F6 F7 FB 2# $ % & * 3 4 5 6 7 9 W E R Y U CO
Which of the following statements is false? When K >> 1, the forward reaction is favored and essentially goes to completion. When K > 1 implies that the reaction is very fast at producing products. None of the above.
Here is a possible reaction: H₂O + NH3 ⇒ NH4* + ¯OH In the space below draw out the full reaction using full Lewis structures and curved arrows to show the movement of electrons. The pka of H₂O is 15.7, and the pKa of NH4* is 9.24. Do you think the reaction mixture at equilibrium will contain: GT 9 mostly products mostly reactants equal amounts of both
Reaction 1: CO(g)+3H2(g)⇄CH4(g)+H2O(g)CO(g)+3H2(g)⇄CH4(g)+H2O(g) K1=[CH4][H2O][CO][H2]3K1=[CH4][H2O][CO][H2]3 Reaction 2: CO2(g)+H2(g)⇄CO(g)+H2O(g)CO2(g)+H2(g)⇄CO(g)+H2O(g) K2=[CO][H2O][CO2][H2]K2=[CO][H2O][CO2][H2] Reaction 3: CH4(g)+2H2O(g)⇄CO2(g)+4H2(g)CH4(g)+2H2O(g)⇄CO2(g)+4H2(g) K3=?K3=? The chemical equations and equilibrium expressions for two reactions at the same temperature are given above. Based on the information, which of the following expressions can be used to calculate the value of K3K3 for reaction 3 at the same temperature? A
10. For the following reactions, circle the more stable cation. Chemical reactions prefer to make more stable products, redraw equilibrium arrows to show the reaction favors the more stable cation. нн N. нон + H-0-н Н. H I N ΗΗ + H но н H O H `N
please indicate the explanation too, thank you

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