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Would this reaction have more products or reactants at equilibrium?
H2PO4- + NH3 ⇌ NH4+ + HPO42-
7.2 36 9.8 12.3 - (pka)
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- What is the concentration of H2C2O4 at equilibrium if I started with .4 M? (Of course the reaction is with wter) Ka1=7.00E-02) Answer: 2.64E-01 M How do we get to that answer step by step?Given the reaction A + B ↔ C + D, which value of Keq MOST strongly favors the production of C + D? A Keq = 1 * 10-3, because the product of the concentration of reactants is more than the product of the concentration of the products. B Keq = 1, because the product of the concentration of reactants is equal to the product of the concentration of the products. C Keq = 1 * 1030, because the product of the concentration of reactants is more than the product of the concentration of the products. D Keq = 1 * 103,because the product of the concentration of reactants is less than the product of the concentration of the products.At equilibrium in the reaction: 4HCl (g) + O2(g) <----> 2Cl2 + 2 H2O if Keq is 4.5 x 10-16 and Cl2= 4M; H2O=5M and HCl=2M what is the conc of O2. pls answer 2 decimals pls thank u
- 12. 2HBr ⇆ H2 + Br2 What will happen to the equilibrium above if H2 is removed from the reaction vessel?2HBr --><-- H2 + Br2 what will happen to the equilibrium above is H2 is removed from the reaction vessel?What does a value of K eq greater than 1 mean?A. More reactants than products exist at equilibrium.B. More products than reactants exist at equilibrium.C. The rate of the forward reaction is high atequilibrium.D. The rate of the reverse reaction is high atequilibrium.
- X <-> Y Keq = 5.66. If the initial concentration of X = 0.1M, what is the concentration of X and Y at equilibrium?1. a) Give the expression for the Ka for each of the following reactions H2CO3 + H2O <=> H3O^+1 + HCO3 ^-1 Ka = H2CO3 + 2 H2O <=> 2 H3O^+1 + CO3^ -2 Ka = b) Give the expression for the Kb for each of the following reactions HCO3^ -1 + H2O <=> OH-1 + H2CO3 Kb = HPO4^ -2 + H2O <=> OH^-1 + H2PO4^ -1 Kb =Calculate the [OH-] at equilibrium for the following reaction starting with [(CH3CH2)2NH] = 0.150 M and no products. ( approximation method) (Answer has 2 sig figs) (CH3CH2)2NH (aq) + H2O(l) <--> (CH3CH2)2NH2+ (aq) + OH- (aq) Kc = 8.6 x10-4
- The Keq for the reaction: A + B <--> AB is 3.013 What is the Keq for 3 + AB <--> 3 A + 3 BFor the reaction - what effect would adding large amounts of heat have on the equilibrium? (Which way would it shift and why?) Explain in terms of LeChatelier’s Principle. Fe3O4(s) + 4 H2 (g) <_-> 3 Fe (s)+ 4 H2O (g) ΔH = 36 kcal Keq = 2.3 x 10-18 During the process of ketogenesis in the liver, 3-hydroxybutyric acid and acetoacetic acid are in equilibrium with each other. However, acetoacetic acid can decompose to form carbon dioxide and acetone in a nonreversible reaction. Answer the following by using LeChatelier’s Principle. What effect would the nonreversible decomposition of acetoacetic acid have on the equilibrium between 3-hydroxybutyric acid and acetoacetic acid? (i.e. which way would if shift?) What effect would the nonreversible decomposition of acetoacetic acid have on the concentration of 3-hydroxybutric acid? (i.e. would it go up or down)5. At 25°C, calculate the molar H3O+ and OH-1 concentrations of the following:b. 0.0600 M NH3c. 0.200 M C6H5COONa (sodium benzoate)d. 0.0860 M KOHe. 0.0689 M HCl
