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...
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At a loss on how to solve these. Have checked my resources and cannot find any explanation. Please help.
![3. If the Keg = 1000 at 50°C and the initial concentration of [FeSCN2'] = 1.00 M, what are the equilibrium
concentrations of [Fe*], [SCN], and [FESCN2']?
4. If the Keg = 10 at 10°C and the initial concentration of [FESCN?*] = 1.00 M, what are the equilibrium
concentrations of [Fe3+], (SCN-], and [FESCN2+]?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c905f52-5d50-40e3-9c88-1b0d49de5da1%2F172eed7c-7e57-46f6-b61d-d7b95a90879a%2F80uy6l_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. If the Keg = 1000 at 50°C and the initial concentration of [FeSCN2'] = 1.00 M, what are the equilibrium
concentrations of [Fe*], [SCN], and [FESCN2']?
4. If the Keg = 10 at 10°C and the initial concentration of [FESCN?*] = 1.00 M, what are the equilibrium
concentrations of [Fe3+], (SCN-], and [FESCN2+]?
![Jltra-bright F
play and auc
Bang & Oluf-
Introduction
The equilibrium state of a chemical reaction can be characterized by quantitatively defining its equilibrium
constant (Kea). In this experiment simulation, you will determine the value of Kea for the reaction between
iron (III) ions (Fe3+) and thiocyanate ions (SCN).
Fe3+ (aq) + SCN (aq)
FESCN2+ (aq)
When you mix amounts of Fe3+ and SCN, a reaction occurs to produce FeSCN2+, but not all of the reactants
react. Thus, at equilibrium, the mixture will contain some of each of these three species. One of the more
important numbers that help us understand an equilibrium system is called the equilibrium constant (Keg).
For the reaction between Fe3+ and SCN, the Keg is defined by the following equation:
[FESCN2+]
[Fe3+][SCN¯]
Kea
In this experimental simulation, you will run several trials of the reaction with differing concentrations of
Fe3*, SCN", and FeSCN2* to determine the equilibrium constant (Keg) for this reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c905f52-5d50-40e3-9c88-1b0d49de5da1%2F172eed7c-7e57-46f6-b61d-d7b95a90879a%2Fp3t56eq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Jltra-bright F
play and auc
Bang & Oluf-
Introduction
The equilibrium state of a chemical reaction can be characterized by quantitatively defining its equilibrium
constant (Kea). In this experiment simulation, you will determine the value of Kea for the reaction between
iron (III) ions (Fe3+) and thiocyanate ions (SCN).
Fe3+ (aq) + SCN (aq)
FESCN2+ (aq)
When you mix amounts of Fe3+ and SCN, a reaction occurs to produce FeSCN2+, but not all of the reactants
react. Thus, at equilibrium, the mixture will contain some of each of these three species. One of the more
important numbers that help us understand an equilibrium system is called the equilibrium constant (Keg).
For the reaction between Fe3+ and SCN, the Keg is defined by the following equation:
[FESCN2+]
[Fe3+][SCN¯]
Kea
In this experimental simulation, you will run several trials of the reaction with differing concentrations of
Fe3*, SCN", and FeSCN2* to determine the equilibrium constant (Keg) for this reaction.
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