Question 26: Which of the following is the closest to the value of K for this reaction? ○ 1.04 9.69E15 1.03E-16 ○ 0.964 Check Reuse <> Embed H-P
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- Given that the Ka for HOCl is 3.5 10-8, calculate the K value for the reaction of HOClwith OH- at 25oC.← < TETNS B Q CAN …. https://app.101edu.co [H3O+] O 2[H3O+] Кс Question 8 of 11 Construct the expression for Kc for the following reaction. CH3COOH(aq) + H₂O(1) ⇒ CH³COO¯(aq) + H³O*(aq) [H3O+]² = Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. X 2[H3O+]² [H₂O] Q Q [H₂O]² h |a|a|Q| + 2[H₂O] RESET 2[H₂O]²2 [CH3COO-] 2[CH3COO-] [CH3COO-]² 2[CH3COO-1² [CH3COOH] 2[CH3COOH] [CH3COOH]² 2[CH3COOH]² T x + ⠀ SubmitCan i get help with E,f, and g
- From the table, what overall conclusions can you make about the direction of equilibrium shift in this reaction? Are your observations consistent with Le Chatelier’s principle?4.) For the following equilibrium reaction state what happens when the following reagents are added NaOH(aq) + HСІ(ад) + НОН(аq) + NaCI(aq)+д a.) Mg(ОН)2 b.) КCІ с.) KBr d.) Heat (A) e.) CH;CH,COH (an acid) f.) decrease in temp.The following equilibrium constants have been determined for hydrosulfuric acid at 25oC ; H2S(aq) ↔ H+(aq) + HS-(aq) Kc’ = 9.5x10-8 HS-(aq) ↔ H+(aq) + S2-(aq) Kc’’ = 1.0x10-19 Calculate the equilibrium constant Kc for the following reaction at the same temperature. H2S(aq) ↔ 2H+(aq) + S2-(aq) 8x10-18 5x10-27 4x10-16 8x10-25 9x10-24
- 6) When the reversible reaction HC;H;O2 (aq) E> H*(aq) + C2H3O2(aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of solid acetate (C2H30,Na) to the reaction mixture? a) pH will not change because C2H;O,Na is not a part of the reaction equation. b) pH will not change because acetic acid and sodium acetate form a buffer c) pH will decrease because the reaction will shift towards reactants d) pH will increase because the reaction will shift towards reactantsagy-m ince Mo atalyst- is catal aw (sin tion of di of gas tv int fors of Co₂ find s :3 S PM" marin what! @ 259 -075 10) The following reaction is known as the Fischer Esterification. The equilibrium constant is 1.0. سال H3C H = + CH₂OH H3C CH3 methylacetate + H₂O a) Write the equilibrium equation for this reaction. However, keep H₂O in the equation. b) With an equilibrium constant of 1.0, what is the maximum yield of the methylacetate product? c) Describe how using Le Chatelier's principle one can increase the yield of the reaction by removing water. 8Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0363 M methylamine (CH, NH,) solution. The Kp of CH, NH, is 4.47 × 10 1. pH (CH, NH, %3! M [CH, NH;] !!
- 6-39. An acidic solution containing 0.010 M Lat is treated with NaOH until La(OH), precipitates. At what pH does this occur?What is the correct equilibrium constant expression for the following reaction? NH3(aq) + H₂O(NH4+ (aq) + OH(aq) [NH3] [H₂O] [NH4]+[OH]- (A) Kc = (B) K (C) Kc (D) Kc (E) Kc = = = = - [NH₂+] [OH-] [NH3] [NH4+] [OH [NH3] [H₂O] [NH3] [NH4+] [OH [NH₁+]+[OH-] [NH3]Fill in the correct “changes” in concentration terms for the following unbalanced equations, (e.g. “+y”, “-2y”, shown in bold in the Ex.) etc, in order to establish equilibrium.NOTE: if you start with a species on the product’s side, that side must lose an amount. Const. T & P. Example: 2 SO3ó 2 SO2 + Cl2(IS balanced) “x” “x” Change: +2y -2y -y a)CH4(g) + O2(g) ó CO2(g) + H2O(g)(unbalanced) “x”“x” Change:_______________ ______ b)H2O(g) + ó H2(g) + O2(g)(unbalanced) “x” “x” Change:__________ ______
