2. Which way will the equilibrium shift (left or right) in the reaction below: Fe3+(aq, yellow) + SCN-(aq) FeSCN2+(aq, red) + heat a. When more SCN-ion (in the form of KSCN) is added to the reaction mixture? Explain why. HINT: Addition of reactants shifts equilibrium toward product; addition of product shifts equilibrium toward reactant. 87

2. Which way will the equilibrium shift (left or right) in the reaction below: Fe3+(aq, yellow) + SCN-(aq) FeSCN2+(aq, red) + heat a. When more SCN-ion (in the form of KSCN) is added to the reaction mixture? Explain why. HINT: Addition of reactants shifts equilibrium toward product; addition of product shifts equilibrium toward reactant. 87

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

Pls help ASAP
2H2O ⇆ H3O+ + OH- To decrease the concentration of OH- ions in the equilibrium above, you could a. add an acid to the solution b. add a base to the solution c. add a catalyst to the solution d. more than one choice is correct
33. What property of a reaction can we use to predict the effect of a change in temperature on the equilibrium constant? lowing re 1217 estamar
please help me with this problem
Calculate the value of equilibrium constant Kc when: a. N2 reacts with O2 to produce NO. At equilibrium, the concentrations of each gas were found to be N2= 0.45M, O2= 0.88M, and NO= 0.98M.
Hemoglobin (Hb), carries oxygen from our lungs to the rest of out body. The figure below shows oxygen binding to the active site of Hb.ONON Fe NNN NCarbon monoxide is poisonous because it binds to Hb in a similar fashion and can displace oxygen and block O2 from binding to Hb.a) The reaction below describes the equilibrium for the displacement of O2 in the HbO2 complex by CO to form HbCO. Write an equilibrium expression for this reaction.HbO2 + CO HbCO + O2Kdisp = ______________b) The equations below describe the equilibrium for O2 and CO binding to Hb. Using the information provided determine the value of KdispHb +O2 HbO2?"#= [???#]=3.2 [??][?#] Hb + COHbCO ?$"= [????]=750 [??][??] 16 Initials __________c) Use your Kdisp to calculate ΔGo for the displacement reaction at 298 K.d) The kinetics of CO displacement of O2 were studied under equal concentrations of each gas at a variety of temperatures. A plot of lnkdisp vs 1/T is shown below, use this information to calculate the…
Write the expression for the Using the equilibrium constant expressions you determined in column 1, Calculate the value of Keg when the following concentrations are present: equilibrium constant Ke, for the reaction below: 3. H20(1) 2 H-(ag) + OH-(ag) [H-]=1x10-8M; [OH-]=1x10-6M; [H2O]=1x10-14M
The following reaction has reached equilibrium, CH3COOH(ag) + H2O(l) ⇄ H3O+(aq) + CH3COO‐(aq) Which way would the reaction go to re‐gain equilibrium if a. CH3COO‐ was added? b. HCl was added (source of H3O+)? c. NaOH was added (source of OH‐ that will react with H3O+)?
A student determines [FeSCN2+] is 0.00016 M at equilibrium. If the initial concentration of Fe3+ was 0.00080 M and the initial SCN- concentration was 0.0012 M, what is the measured value of Kc?
Consider the following equilibrium reaction: Cu+2 (aq) + 2 Ag (s) = Cu (s) + 2 Ag*1 (aq) What is the Kc expression? Select one: [Ag+1]² [Cut2] O a. Ke [Ag+1] O b. K. = [Cut2] [Cut2] [Ag+1]² ,+2 O c. Ke = [Ag+1]*[Cu] [Cu+2][Ag]? O d. Ke [Cu+2] [Ag+1] O e. Kc
See attached files. question : For reaction 5, Step 17, explain why the equilibrium shifted to the right.
Select the statement that best describes what happens when the concentration of PbO is decreased:PbO(s)+NaCl(aq)+H2O(l)↔Pb(OH)Cl(s)+NaOH(aq) a. The reaction will shift to the left thereby increasing the concentration of the reactants to restore equilibrium. b. The reaction will shift to the left thereby increasing the concentration of the products to restore equilibrium. c. The reaction will shift to the right thereby increasing the concentration of the reactants to restore equilibrium. d. The reaction will shift to the right thereby increasing the concentration of the products to restore equilibrium. e. No Change.