Apply Le Chatelier's principle to determine the equilibrium shift of the following reaction under different conditions: A(ac) + B(aq) → 3C(ac) Conditions Answer A concentration increases B concentration increases B concentration decreases A concentration decreases The concentration of B triples and the concentration of C triples C concentration increases C concentration decreases The concentration of A triples but the concentration of B decreases to a third Options Equilibrium shifts to the right There's no change Equilibrium shifts to the left ●

Apply Le Chatelier's principle to determine the equilibrium shift of the following reaction under different conditions: A(ac) + B(aq) → 3C(ac) Conditions Answer A concentration increases B concentration increases B concentration decreases A concentration decreases The concentration of B triples and the concentration of C triples C concentration increases C concentration decreases The concentration of A triples but the concentration of B decreases to a third Options Equilibrium shifts to the right There's no change Equilibrium shifts to the left ●

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section: Chapter Questions

Problem 48GQ: In the gas phase, acetic acid exists as an equilibrium of monomer and dimer molecules. (The dimer...

See similar textbooks

Similar questions

. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.
In the gas phase, acetic acid exists as an equilibrium of monomer and dimer molecules. (The dimer consists of two molecules linked through hydrogen bonds.) The equilibrium constant, Kc, at 25 C for the monomer-dimer equilibrium 2 CH3CO2H (CH3CO2H)2 has been determined to be 3.2 104. Assume that acetic acid is present initially at a concentration of 5.4 104 mol/L at 25 C and that no dimer is present initially. (a) What percentage of the acetic acid is converted to dimer? (b) As the temperature increases, in which direction does the equilibrium shift? (Recall that hydrogen-bond formation is an exothermic process.)
Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide.NH4I(s) ↔ NH3(g) + HI(g)At 400°C, Kp = 0.49. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
Given the following reaction at equilibrium, if Kc = 5.94 x 105 at 230.0 °C, Kp = ________.2NO (g) + O2 (g) 2NO2(g) A. 6.44 ⋅ 105 B. 2.45 ⋅107 C. 3.67 ⋅ 10-2 D. 1.44 ⋅ 104 E. 2.44 ⋅ 106
The reaction: Fe3+(aq) + SCN- (aq) ⇌ FeSCN2+(aq) is an equilibrium reaction that produces a colored product, atequilibrium the reaction is an orange color. The complex ion FeSCN2+(aq) is a very dark reddish brown,while the reactant Fe3+ is a very pale yellow and SCNis colorless.Starting with a system at equilibrium, predict the change to the color when the following take place.A) More Fe3+ is added B) HPO42-(aq)was added and precipitated the Fe3+(aq) ions as Fe2(HPO4)3(s).
At 292.8 oC, the Keq for the reaction is 4.23⋅ 10-5: 3 A + 5 B ↔ 1 AB What is Kp?
At 2200°C, Kp = 0.050 for the reaction N2(g) + O2(g) ↔ 2NO(g) What is the partial pressure of NO inequilibrium with N2 and O2 that were placed in flask at initial pressures of 0.80 and 0.20 atm, respectively
1.40 moles of H2O2 were placed in a 2.00 L reaction chamber at 307ºC. After equilibrium was reached, 0.96 moles of H2O2 remain. Calculate the equilibrium constant, Kc, for the reaction: 2H2O2 (g) ⇄ 2H2O(g) + O2 (g) Please outline step by step how do this problem and the formulas used
The binding of oxygen by hemoglobin (Hb), giving oxyhemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized asHbO2(aq) + H3 O+(aq) + CO2(g) ⇌ CO2 −Hb−H+ + O2(g) + H2 O(i)(a) Write the equilibrium constant expression for this reaction.(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxyhemoglobin in the blood passing through the muscle.
10. In Part D, what property will you observe that will allow you to determine the direction of equilibrium shift for the reaction Fe3+(aq) + SCN-(aq) = FeSCN2+(aq)
In the given laboratory activity on the concentrations and temperature effects on equilibrium, thegiven aqueous reaction were observed:Fe -3 + SCN°+ FeSCN 2(light yellow) + (deep Red) Use your knowledge in equilibrium, which of the following will be produced if Fe(NO3)3 will be addedinto the given aqueous reaction.A. The color in the test tube will become a deeper red color because the equilibrium will shift tomake more reactants.B. The color in the test tube became a deeper red color because the equilibrium shifted to makemore products.C. The color in the test tube became a lighter color because the equilibrium shifted to make morereactants.D. The color in the test tube became a lighter color because the equilibrium shifted to make moreproducts.
The following reaction has Kp = 109 at 25°C. 2 NO(g) + Br2(g) 2 NOBr(g) If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.