Part ACalculate the value of K_eq from the following equilibrium concentrations: [FeNCS²+]=1.42x10-4 M , [Fe³+]=8.62x10-4 M , and [SCN¯]=4.89×10-4 M.| ΑΣφSubmitPrevious Answers Request AnswerX Incorrect; Try Again; 2 attempts remaining

Equilibrium is a state in a reaction that is achieved when the rate of the forward reaction becomes…

Answered: Calculate the value of K_eq from the…

Calculate the value of K_eq from the following equilibrium concentrations: [FeNCS²+]=1.42×10M , [Fe³*]=8.62x10-4 M , and [SCN¯]=4.89x10¬4 M .

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 76QAP

See similar textbooks

Related questions

Q: onstruct the expression for Kc for the llowing reaction. 2 Ag(s) + Zn*(aq) =2 Ag*(aq) + Zn(s) 1 Drag…

Q: Express the equilibrium constant for the following reaction. N2(g) +3 H2(g) = 2 NH3(g) N2][H2]1/3 K…

A: Given N2(g) + 3H2(g) →2(NH3)(g) we need to find equilibrium constant K

Q: What would be the equilibrium constant expression for the following equations? Br2(g) +…

Q: Suppose that the equilibrium constant for chemical reaction 2A><B is 2.3 x 10^7, what is the…

Q: At 800 K, the equilibrium constant for the reaction A2(g) = 2A(g) is Kc = 3.1 * 10-4. If the value…

Q: Calculate the analytical and equilibrium molar concentrations of the solute species in an aqueous…

A: Mass of trichloroacetic acid = 285 mg Molar mass of trichloroacetic acid = 163.4 grams Number of…

Q: Write equilibrium expressions for the following equilibria: a) Ka1 and Ka2 for the dissociation of…

Q: Write the equilibrium-constant expression for the following reaction: 2NO (g) + 2H2 (g) ↔↔ N2 (g)…

A: Given reaction at equilibrium: 2NO (g) + 2H2 (g) ↔ N2 (g) + 2H2O (g) We have to write the…

Q: At 25 °C, an aqueous solution has an equilibrium concentration of 0.00357 M for a generic cation,…

Q: The ionization constant (K») of aniline (CsHsNH2) is 2.35 x 10-5, If 7.285 grams of aniline is…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Write the equilibrium constant for 3NO(g) ↔ N2O(g) + NO2(g

A: Chemical equilibrium is the state of a system in which the reactant and agent concentrations do not…

Q: Write equilibrium expressions for the following gas-phase reactions. = 2 Cl½O(g) (a) 2 Cl2(g) +…

Q: The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10 and a professor made 1825 mL of a CaSO4(aa)…

A: The question is based on the concept of Le-chatlier principle. It States that when a system at…

Q: Write the equilibriu

A: 1 . magnesiumhydoxide is sparingly soluble salt , whenit is dissolved the following equilibrium is…

Q: What is the equilibrium constant expression for: 4 NH3(g) + 502(g) = 4 NO(g) + 6 H20(1) NH33[022…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

A: Reaction of solubility of M(OH)2 in water M(OH)2 (aq) →M2+(aq) + 2 O-H (aq)pH of solution 10.36pH +…

Q: The acid-dissociation constant for benzoic acid (C6H5COOH)is 6.3 x 10-5. Calculate the equilibrium…

A: The dissociation reaction of C6H5COOH is as shown below => C6H5COOH (aq) + H2O (l) ------>…

Q: 1) Write the equilibrium constant expression for the dissociation of acetic acid

A: Below attached file showing the details answer. All the best. As per Bartleby answering guidelines…

Q: For the reaction 4 PH, (g) = 6 H, (g) + P,(g) the equilibrium concentrations were found to be [PH,]…

Q: (a) Write down the overall reaction for the formation of the complex ion [Zn(NH:)-]²*(aq) from its…

Q: Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and…

Q: 6. Calculate the equilibrium [Fe3*] in each mixture. a. 60.0 mL of 0.0200 M Fe(NO3)3 is combined…

A: #(6) #(a): Balanced equation for the formation of Fe(CN)63-(aq) is Fe3+(aq) + 6 CN-(aq)…

Q: Write the expression for the equilibrium constants for the following reactions. FeCl3 (s) Fe+ (aq) +…

Q: Starting with 0.0116 M Cu2* and 0.230 M NH3 and forming Cu(NH3)42+ ion (Kf = 1.10x1013), determine…

Q: Find the equilibrium constant for the reaction Nas) + Fe3+= Fe²+ + Na+

A: Equilibrium constant (Keq) is the ratio of the concentration of products to the concentration of…

Q: Write the equilibrium constant expression, Kc, for the following reaction: (If either the numerator…

Q: Write the equilibrium constant expression and the value of k for the following reactions: N2(g) +…

Q: 5. Write forward and reverse reactions for the following: CH4 (g) + 2H2S (g) (g) ==== CS2 (g) + 4H2…

Q: 2. Calculate the equilibrium constant, K, for the reaction: SOz1e) + Oz(e) > SO31e) Given: [SO3] = 5…

Q: Write the equilibrium constant expression for this reaction: 2 CH₂COO (aq) + C₂H₂O₂(aq) →…

Q: Calculate the concentration of free, uncomplexed Cu2+ ions in a solution that originally contains a…

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: Write the dissociation reaction and the corresponding K equilibrium expression for HCN

A: As per the question dissociation reaction and equilibrium constant expression for weak acid HCN are…

Q: Write the following equilibrium-constant expressions: Kc for Cr(s) + 3 Ag+(aq) <=> Cr3+(aq) +…

A: Given chemical reactions are in heterogeneous equilibrium, and asked to write the corresponding…

Q: Consider the reversible dissolution of lead(II) chloride. Suppose you add 0.2429 g of PbCl2(s) to…

A: The dissolution reaction of PbCl2 is => PbCl2 (s) ------> Pb2+ (aq) + 2 Cl- (aq)

Q: Write the equilibrium constant for the following reactions: a. 3NO(g) ↔ N2O(g) + NO2(g) b.…

A: The equilibrium constant for the reactions has to be written. Equilibrium constant expression is not…

Q: For the reaction, 2NH3(g)--> <---3H2 (g)+ N2 (g) the equillibrium concentrations were found to be…

A: The reaction given is 2NH3(g)--> <---3H2 (g)+ N2 (g) Hence the equilibrium constant…

Q: e) [H] = 0.0045 M, [Cl,] = 0.0045 M, [HCI] = 0.0625 M

Q: The equilibrium constant, K, for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g) +…

A: Given, Kc = 1.80*10-4

Q: 1. In this experiment we measured K, for borax Na,B,0,(OH), 8H,0(s)=2Na*(aq)+ B,0,(OH),¯(aq)+8H,0(1)…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: The equilibrium constant, K, for the following reaction is 1.77x10 3 at 568 K. NH4CI(s) NH3(g) +…

A: Kc is equilibrium constant and Kc is equal to ratio of concentration of product and concentration of…

Q: 2 C₂H₂(g) + 2 H₂O(g) → 2 C₂Hs(g) + O₂(g)

A: Kc = [C2H6]2[O2] / [C2H4]2[H2O]2

Q: 3. The solubility product constant (Ksp) of iron (III) chloride is 1.7 x 10-6. Calculate the molar…

A: The molar solubility of a compound is the concentration of any substance in its saturated solution.…

Q: The equilibrium constant, Kc, for the following reaction is 1.20x10-2 at 500 K. PCI5(g) PCI3(g) +…

A: All data mentioned in handwritten solution.

Q: Given the following values of equilibrium constants: [Ag(NH, )2]* = Ag (aq) + 2NH3(aq) K = 6.3 ×…

A: We are given the following two reaction: [Ag(NH3)]2+⇌Ag+(aq)+2NH3(aq)…

Q: What is the equilibrium constant expression for the reaction: 3 Fe(s) + 4 H2O (g)⟷ Fe3O4 (s) + 4 H2…

A: Given :- 3 Fe(s) + 4 H2O (g)⟷ Fe3O4 (s) + 4 H2 (g) To write :- Equilibrium constant expression…

Q: 4. Calculate the equilibrium concentrations of hydrogen & and iodine that result when 0.050mol HI is…

Q: For the synthesis of ammonia from its elements, 3 H2(g) + N2(g) 2 2 NH;(g)

A: Equation used to calculate the standard Gibbs free energy change of the reaction is:…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Part A
Calculate the value of K_eq from the following equilibrium concentrations: [FeNCS²+]=1.42x10-4 M , [Fe³+]=8.62x10-4 M , and [SCN¯]=4.89×10-4 M.
| ΑΣφ
Submit
Previous Answers Request Answer
X Incorrect; Try Again; 2 attempts remaining

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Answer

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
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?