10. The expression Kc = 2 × [H+]2 × [C2O42–] / [H2C2O4] corresponds to which reaction in aqueous solution?
(A) 2 H+ + C2O42– H2C2O4
(B) H2C2O4 2 H+ + C2O42–
(C) H2C2O4 H+ + HC2O4–
(D) H2C2O4 H+ + C2O42–
(E) None of these
***Can someone explain the answer to me?
10. The expression Kc = 2 × [H+]2 × [C2O42–] / [H2C2O4] corresponds to which reaction...
Can somebody work through this problem for me? Consider an aqueous solution of oxalic acid (H2C2O4), used in bleaching leather and removing rust and ink strains. What is the pH and [C2O42– ] in a 0.15 M H2C2O4 solution (Ka1= 6.5 × 10–6; Ka2 = 6.1 × 10–10)? (The answer is 3.0 and 6.1 × 10–10)
For a simple reaction, A ↔ B, the expression for the equilibria is Kc = [B]/[A]. Which term(s) in the expression are variable? a. Kc b. [B] c. [A] d. [A] & [B] e. Kc & [A] & [B]
Q(22) Kp=Kc when? A) The reaction is at equilibrium B) The reaction is exothermic C) The reaction is endothermic D) all of the gasses present are at the same temperature E) the number of moles of gas on both sides of the balanced equation is the same. Q(23) HAH +A at the equilibrium (HA) = 1.65* 10-2 M and [H") = (A-) = 5.44*10-4 M at equilibrium. Kc = A) 1.7 X 10-1 C) 1.7 X 103 D) 1.7 X...
2 HgCl2(aq) + C2O42-(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) Experiment [HgCl2], M [C2O42-], M Initial rate 1 0.105 0.15 1.8 x 10-5 2 0.105 0.30 7.1 x 10-5 3 0.052 0.30 3.5 x 10-5 4 0.052 0.15 8.9 x 10-6 a) Determine the order of reaction with respect to HgCl2. b) Determine the order of reaction with respect to C2O42-. c) Determine the overall order of the reaction. d) What is the rate law? e) Determine the...
ZnO is) + H2g) ² Znis) + H₂Oig) Which is the correct equilibrium constant expression for the following reaction. a) Kc=[H₂O] / [H2 ] b) Kc = [Zn] [H₂O] / [ano] c) Kc = [ zno] [ H₂] / [an] [ H₂O] d) Kc =[ zn] [H₂O]/[ano] [ H₂] el Kc = [Hz ] /[H₂O]
The reactions below are all at equlibrium simultaneously in solution: 1. Ca^2+(aq) + C2O4^2- (aq) --> <-- CaC2O4 (s) 2. H2C2O4 (aq) --> <-- H+ (aq) + HC2O4 -^ (aq) 3. HC2O4^- (aq) --> <-- H^+ (aq) + C2O4 ^2- (aq) a. If potassium hydroxide is added to this solution, would you expect to see more or less of the precipitate (CaC2O4) formed in the solution? Explain your reasoning by showing the effect of the addition of potassium hydroxide on...
Vrite a balanced chemical equation which corresponds to the following equilibrium constant expression. [NO] H₂O K = (HNO2) Select one: a. HNO3(aq) - H20(8)=NO:"(aq) - H30"(aq) b. NO:- (aq) - H30"(aq) = HNO2(aq) - H.0() C. NO:- (aq) - H30 (aq) = HNO3(aq) d. HNO3(aq) =NO: (aq) - H:0"(aq) e. H(aq) - OH (aq) =H-08) die good die Ware about our
Consider the Reaction A+B <--> C+D, which has an equilibrium constant, Kc = 3.4 x 10^2. If one begins a reaction by placing 0.600 moles of A in a 1.0L container as well as 0.150 moles of B, what will be the equilibrium concentrations of A, B, C, D? Write your answer in the spaces below. a. [A] = ______ b. [B] = ______ c. [C] = ______ d. [D] = ______
The equilibrium constant kc for the reaction N2(g)+3H2(g) ⇌ 2NH3(g), which corresponds to the formation of ammonia by the Haber process, is 2.13 x 106 at 288k and 1.75 x 105 at 308 k. Calculate the standard enthalpy at 298k Answer: -92,2 kJ/mol
2) For the chemical reaction CO2(g) + H2O(0) - H:CO3(aq) give the correct expression for Kc, Kp, and K, or explain why such an expression cannot be given.