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Calculate delt G for
a.) CH3NH2(aq) + H2O (l) -> CH3NH3+ (aq) + OH-(aq)
T= 25C
kp= 4.4x 10-4
b.) Pbl2(s) + Pb2+(aq) +2I-(aq)
T= 25C
Kp= 8.7x10-9
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- O Ni(H₂O)2+ (aq) + 3SCN- (aq) = Ni(SCN); (aq) + 6H₂0(1) (a) Write the Kc expression for this equilibrium. (b) Would there be a shift to the right or to the left if KSCN solution was added to a solution containing this equilibrium? Explain your answer.H3O* (aq) + OAC° (aq) Н2о () + НОАc (аq) +» НҙО* (аq) + ОАc" (аq) the Dissociation Constant Ka of HOAC: Ka = [HOAC]/([H30*][OAC¯]) Ka = [H3O*][OAc]/([HOAC][H2O]) Ka = [H3O*][OAc"]/[HOAC] O Ka = [HOAC][H2O]/([H3O*][OAC¯]) %3DThe 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
- The Ksp for SrF2 is 2.45 x 10-9. Use this information to calculate the solubility of Strontium Fluoride in water (find the [Sr2+] and [F-] at equilibrium). SrF2 (s) Sr2+ (aq) + 2F- (aq) I C EC=a4bc46ac4 Part A X Given the two reactions 1. H₂S(aq) = HS (aq) + H+ (aq), K₁=9.46x10-8, and 2. HS- (aq) = S²-(aq) + H+ (aq), K2 = 1.31x10-19, what is the equilibrium constant Kfinal for the following reaction? DO Enter your answer numerically. ► View Available Hint(s) Kfinal Submit W LIVE ΑΣΦ MacR Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions Contact Us D P Pearson zoom S² (aq) + 2H+ (aq) = H₂S(aq) t O ? ReviewCalculate the equilibrium constant (Kc) for the following reaction: CH3COOH(aq) + OH-(aq)) CH3COO-(aq) + H2O(l) The Ka of acetic acid is 1.75 x 10-5; Kw for auto-ionization of water = 1 x 10-14 Hint: First write the equilibrium expressions for both species (reactants) separately then apply manipulation rules of K and find the answer)
- 0.00130 molk (CH2)NH* POH = - log (u.8x 10-5) - log (0.8x 10-s) 4.50 + 20.0D = 214.50 x 10-3L log 0.00110 mols (CH)N 24.50 x 10-3LThe following reactions all have K < 1. 1) CIЮ (aq) + СGH;ОН (аq) — HCIO (аq) + СoH;0 (аq) 2) HCOO (aq) + C6H5OH (aq)=C;H5O° (aq) + HCOOH (aq) 3) HCIO (aq) + HCОО (аq) НСООН (аq) + CIO- (аg) Arrange the substances based on their relative BASE strength. Clear All CIO C,H30 strongest base C,H5OH intermediate base НСООН weakest base НСО- not a Bronsted-Lowry base HCIOGiven the following two equilibria at 750 K. NiCO3 (s) ⇔ Ni2+(aq) + CO32-(aq) Kc = 6.6 x 10-9 HCO3- (aq) + H2O(liq.) ⇔ CO32- (aq) + H3O+ (aq) Kc = 4.8 x 10-11 Based on the above two equilibria, calculate the equilibrium constant for the following reaction at 750 K. NiCO3(s) + H3O+ (aq) ⇔ Ni2+(aq) + HCO3- (aq) + H2O(liq.
- The following reactions all have K <1. 1) HCOO" (aq) + HCN (aq) HCOOH (aq) + CN (aq) 2) CN (aq) + CH;OH (aq) HCN (aq) + CH3O" (aq) 12 3) C,HgOH (aq) + HCOO (aq) C&HgO (aq) + HCOOH (aq) Arrange the substances based on their relative BASE strength. Clear All CN strongest base HCN intermediate base CH3OH weakest baseagy-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. 8estion 15 of 22> Given that K for HCN is 6.2 × 10- at 25 °C, what is the value of K, for CN at 25 °C? -10 K = Given that Kp for CH,CH,NH, is 6.3 × 10-ª at 25 °C, what is the value of Ka for CH,CH, NH; at 25 °C? Ka = 13 étv