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- 7:40 session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass :Dcalculate the value of the equilibrium constant, Rc₂ Q (g) + x (g) = 2 M(g) + N(0) given that KC₁ - 3.20 ког = 0.443 14.0 Кез Meg) = 2(g) 6Rcg) = 2 N(g) + 47 (8) 3 X (9) +30)(9) — 9R(g) R= ? GIVE EXPLAINED HANDWRITTEN ANSWERAcetic acid is a weak acid that partially dissociated in water according to equation B1-2, with an acid dissociation constant Ka = 1.66 x10-5: CH3COOH + H₂O CH3COO H3O+ Equation B1-2 d. 0.67 mol of acetic acid are added to 1 litre of pure water with no discernible change in volume. Determine the equilibrium concentrations of acetic acid (CH3COOH), acetate ion (CH3COO-) and hydronium ion (H3O*).formic acid (0.24mol) is placed in 2L of water and undergoes the following reaction:HCHO2(aq)+H2O(l) - H3O+(aq)+ CHO2-(aq) Kc= 2.1*10-4. (a) use your solver to calculate the equilibrium concentration of hydronim ion in this solution? (b) Approximate the answer to this problem by assuming x is small. show your work.› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6Calculate 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)ASAPFor the reaction 3 H2(g) + N2(g) 2 NH3(g), at 472°C equilibrium is established when [H₂] = 0.0200 M, [N₂] = 0.0100 M and [NH3] = 5.37 x 10-8 M. What is the equilibrium constant for this reaction? For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial X² X₂ ¶ ¶< +. RBC V 10pt ✔ ✓ V くく A V AV Ix ¶T 99 Ω ΩΘΑ 田く x 88 H HJ XQ 田田图 883 == E TO) ... xxWrite the equilibrium- constant expression for the reaction A(s)+3B(l) rightleftharpoons2C(aq)+D(aq) in terms of |A|, [B], [C] and [D]as needed. Note that K c , which is sometimes symbolized as K eq , denotes that the equilibrium constant is expressed using molar concentrations. For this question, K c means the same thing as K cqAt 700 K, the reaction 2502(9) + O2(9) = 2503(9) has the equilibrium constant Ke = 4.3 x 106, and the following concentrations are present: [SO2) = 0.010 M: [SO3) = 10. M: [02) = 0.010 M. Which of the following is true based on the above? Multiple Cholce Qc Kc. the reaction proceeds from right to left to reach equilibrium Qc Ke, the reaction proceeds from left to right to reach equiloriumConsider the following equilibrium reaction: Baz(PO4), (s) = 3 Ba2*(aq) + 2 PO,3-(aq) Kc = 3.4 x 10-3 %D 2.00 moles of each reactant and product were placed in 5.00 L of water, mixed and allowed to reach equilibrium. a) Write the Qc expression (LMA) for this reaction. b) Calculate the value of Qc. (Show all work for full credit.) c) In which direction will this reaction proceed to establish equilibrium. Explain your answer. d) Once equilibrium is reached, it was found that the barium ions CHANGED by 0.455 mol. How many moles of each reactant and product are present at equilibrium? (BOX YOUR FINAL ANSWER.)For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.SEE MORE QUESTIONS