Find K and average K **Transcription of Beaker C Equilibrium Experiment Data****Section 3. From Beaker C**| | Fe³⁺ | + | SCN⁻ | ⇌ | FeSCN²⁺ ||----------------------|-----------------------|------------------|---------------------|-----------------|-------------------|| **Initial** | 0.6 x 10⁻³ | | 1 x 10⁻³ | | 0 || **Change** | -9.732 x 10⁻⁵ | + | -9.732 x 10⁻⁵ | | + || **Equilibrium** | 0.898 x 10⁻³ | | 9.732 x 10⁻⁵ | | 0 |**K =** **Average K = ______****Explanation:**This table outlines the changes in concentration of the reactants and products during a chemical equilibrium experiment involving iron(III) ions (Fe³⁺), thiocyanate ions (SCN⁻), and the resulting complex ion (FeSCN²⁺). The concentrations are given in molarity (M).- **Initial Row:** Shows the starting concentrations of Fe³⁺ and SCN⁻, with FeSCN²⁺ initially being 0 M.- **Change Row:** Indicates the change in concentration needed to reach equilibrium. The reactants decrease by 9.732 x 10⁻⁵ M, suggesting formation of FeSCN²⁺.- **Equilibrium Row:** Displays the concentrations when the system reaches equilibrium.The blank areas under “K” and “Average K” are likely for calculating the equilibrium constant (K) based on the given data.

Answered: Image /qna-images/answer/f9241410-7dd2-4ddf-a242-95849a341da0.jpg

Answered: 3. From Beaker C K= Initial Change…

3. From Beaker C K= Initial Change Equilibrium Average K= Fe³+ 0.6x10 3 -9.732x10-5 0.899x103 + SCN 1x10³ +9.732x105 9.73240² FeSCN2+ 0 0 0

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

r. Please dontprovid ehandwriting solution.
At a certain temperature, 0.700 mol SO, is placed in a 2.50 L container. 2 SO3 (g) = 2 S0,(g) + 0,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke =
If the equilibrium constant for a reaction is very large, what is the reaction
Please provide detailed solution and give the explanation of the concept
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 45. mol of ethylene gas and 35. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 34. mol of ethylene gas and 24. mol of water vapor. The engineer then adds another 18. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. | mol
056575718snapshotld=13245488&id-5636490008takeld=4bfba59b09f0e5b& Q Search this course X References Use the References to access important values if needed for this question. Consider the following reaction where K, = 4.55x10 at 723 K: H N2(g) +3H2(g)2NH3(g) 1008 If the three gases are mixed in a rigid container at 723 K so that the partial pressure of each gas is initially one atm, what will happen? A-Z Indicate True (T) or False (F) for each of the following 1. A reaction will occur in which NH (g) is consumed. 2. Kn will increase. 3. A reaction will occur in which N, is consumed 4. Q is less than K. 5. The reaction is at equilibrium. No further reaction will occur 4. Q versus K: This is group attempt 1 of 5 Autosaved at 1:06 PM Back Next 1:06 PM PRA x 11 9/24/2019 Lhp delete 12 prt sc f11 insert KA
Write the K, expression for the sparingly soluble compound copper(II) hydroxide, Cu(OH),. If either the numerator or denominator is 1, please enter 1.
At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increas of moles of gas in the system.
Suppose a 500. mL flask is filled with 0.30 mol of Cl, and 1.2 mol of HCl. The following reaction becomes possible: H,(g) +Cl, (g)- 2HC1(g) (3) 12+ The equilibrium constant K for this reaction is 5.59 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. |M