QUESTION 8 Chemical Equilibrium In this lab, the reaction below was studied. Fe³+ (aq) + NCS- (aq) FeNCS2+ (aq) Colorless Red-Orange In Part A, additional reagents are added to the equilibrium mixture, and the color of the solution is used to qualitatively interpret the "position" of the equilibrium. Which of the following correctly predicts the color change for each given addition? Equilibria.pdf O Added: Fe(NO3)3 (aq) Color Change: Clear to Dark Red-Orange O Added: NaNCS (aq) O Added: Fe(NO3)3 (aq) O Insufficient information O Added: FeNCS²+ (aq) Color Change: Red-Orange to Yellow Color Change: Light Red to Colorless given. Color Change: Clear to Red-Orange

QUESTION 8 Chemical Equilibrium In this lab, the reaction below was studied. Fe³+ (aq) + NCS- (aq) FeNCS2+ (aq) Colorless Red-Orange In Part A, additional reagents are added to the equilibrium mixture, and the color of the solution is used to qualitatively interpret the "position" of the equilibrium. Which of the following correctly predicts the color change for each given addition? Equilibria.pdf O Added: Fe(NO3)3 (aq) Color Change: Clear to Dark Red-Orange O Added: NaNCS (aq) O Added: Fe(NO3)3 (aq) O Insufficient information O Added: FeNCS²+ (aq) Color Change: Red-Orange to Yellow Color Change: Light Red to Colorless given. Color Change: Clear to Red-Orange

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

please answer all
For the reaction 2 NH3 = 3H₂ + N₂ The equilibrium concentrations were found to be [NH3]=0.250 M [H2]=0.450 M [N2]=0.800 M. What is the equilibrium constant for this reaction?
What is the equilibrium concentration for H2O. You are given the initial concentrations for all components. Make sure to determine the proper direction
A. Using the Le Chatelier’s principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied.
Help on these two plz
The precipitation of three solid compounds: X, Y, Z, have the following equilibrium constants: KX = 1.7 x 104 KY = 0.6 x 108 KZ = 9.2 x 1012 Assuming a solution contains equal concentrations of ions to form these compounds, which among the three would have the least amount of precipitate at equilibrium?
The initial concentration of Cl1- is 0.100M and the initial concentration of Co(H2O)62+ is 0.500 M. At equilibrium the concentration of CoCl42- is 0.0035. What is the value of the equilibrium constant for the reaction being studied?
3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN²+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.
Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.
55. Consider the reaction: MISSED THIS? Read Section 16.8; Watch KCV 16.8, WE 16.9 NiO(s) + CO(8) = Ni(s) + CO2(g) K. = 4.0 × 10³ at 1500 K If a mixture of solid nickel(II) oxide and 0.20 M carbon monox- ide comes to equilibrium at 1500 K, what is the equilibrium concentration of CO,2
Given that the maximum concentration of Ag2CrO4 in water is 6.627*10-5 M, determine the solubility product of this equilibrium: Ag2CrO4 ⇆ 2Ag++ Cr(O42-)
A. Using the Le Chatelier's principle, predict the shift in the direction of the equilibrium position and changes that will be observed (e.g. color) in each of the following equilibria when the indicated condition is applied.| 1. Ifheat is added to a phase change equation at equilibrium from solid to liquid, which way will the reaction proceed? 2. In this reaction: H2Om = H2O how could conditions be manipulated to create more H2Qa? 3. Which side is heat on in this reaction (photosynthesis): 6COX + 6H2O@= C¢H12O620) + 60z) 4. Heat + Co+Ca+ 4 Claq) = COC4 ²- caq) when the equilibrium mixture is cooled. (exothermic) pink colorless blue 5. Fet) 6SCNa) - Fe(SCN)6 *w when Fe³+ is added to the equilibrium mixture. brown colorless red