4:03 PM Thu Mar 2[0]Consider the equilibrium systemdescribed by the chemical reactionbelow. For this reaction, Kc = 2.1 x 10³at a certain temperature. If theequilibrium concentrations of H₂ and F₂are both 0.0021 M, determine theconcentration of HF at equilibrium.H₂(g) + F₂(g) 2 HF(g)Kc =[0.0021] 2[0.0021]2[0.0011] [0.0011]³Question 17 of 19If [x] represents the equilibrium concentrationof HF, set up the equilibrium expression for Kcto solve for the concentration. Each reactionparticipant must be represented by one tile.Do not combine terms.Tap here or pull up for additional resources[x]2[2x]NEXT>= 2.1 x 10³[x]²[2x]²SubmitRESET[0.0011]Hydramonoxmixturof 2.00K₂ = 13initialchangeequilibriu

An equilibrium chemical equation is given as follows:The equilibrium constant, Kc for the above…

[0] Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 x 10³ at a certain temperature. If the equilibrium concentrations of H₂ and F₂ are both 0.0021 M, determine the concentration of HF at equilibrium. H₂(g) + F₂ (g) = 2 HF(g) Kc = [0.0021] 2[0.0021] 2[0.0011] [0.0011]' Question 17 of 19 1 If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. R 2 [2x] NEXT> = 2.1 x 10³ [x]² [2x]¹ Submit RESET [0.0011]

[0] Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 x 10³ at a certain temperature. If the equilibrium concentrations of H₂ and F₂ are both 0.0021 M, determine the concentration of HF at equilibrium. H₂(g) + F₂ (g) = 2 HF(g) Kc = [0.0021] 2[0.0021] 2[0.0011] [0.0011]' Question 17 of 19 1 If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. R 2 [2x] NEXT> = 2.1 x 10³ [x]² [2x]¹ Submit RESET [0.0011]

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

See similar textbooks

Similar questions

Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the initial concentration of PCl5 is 0.1000 M, what are the equilibrium concentrations of the reactants and products?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?