Suppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be 9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. 3/3 Fe3+ (aq) SCN (aq FeNCS2+ (aq) Step 1. Calculate the initial number of moles of Fe3+ and SCN (use Equation 12). moles of Fe3+ moles of SCN Step 2. How many moles of FeNCS2+ are present at equilibrium? What is the volume of the equilibrium mixture? mL moles of FeNCS2+ How many moles of Fe3 and SCN are consumed to produce the FeNCS2+? moles of Fe3+ moles of SCN Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa- tion (13) and the results of Steps 1 and 2. moles of Fe3+ moles of SCN 9
Suppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be 9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. 3/3 Fe3+ (aq) SCN (aq FeNCS2+ (aq) Step 1. Calculate the initial number of moles of Fe3+ and SCN (use Equation 12). moles of Fe3+ moles of SCN Step 2. How many moles of FeNCS2+ are present at equilibrium? What is the volume of the equilibrium mixture? mL moles of FeNCS2+ How many moles of Fe3 and SCN are consumed to produce the FeNCS2+? moles of Fe3+ moles of SCN Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa- tion (13) and the results of Steps 1 and 2. moles of Fe3+ moles of SCN 9
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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I have a 3 step problem about Determination of an Equilbrium constant.
![Suppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M
KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be
9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula-
tions for each step.
3/3
Fe3+
(aq)
SCN (aq FeNCS2+
(aq)
Step 1. Calculate the initial number of moles of Fe3+ and SCN (use Equation 12).
moles of Fe3+
moles of SCN
Step 2. How many moles of FeNCS2+ are present at
equilibrium? What is the volume of the
equilibrium mixture?
mL
moles of FeNCS2+
How many moles of Fe3 and SCN are consumed to produce the FeNCS2+?
moles of Fe3+
moles of SCN
Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa-
tion (13) and the results of Steps 1 and 2.
moles of Fe3+
moles of SCN
9](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5db13df0-2ae2-4f45-bd91-780f2de28c1f%2F0aaac1b6-b770-4c62-a879-48d847d45b61%2Ftcrp739.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M
KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be
9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula-
tions for each step.
3/3
Fe3+
(aq)
SCN (aq FeNCS2+
(aq)
Step 1. Calculate the initial number of moles of Fe3+ and SCN (use Equation 12).
moles of Fe3+
moles of SCN
Step 2. How many moles of FeNCS2+ are present at
equilibrium? What is the volume of the
equilibrium mixture?
mL
moles of FeNCS2+
How many moles of Fe3 and SCN are consumed to produce the FeNCS2+?
moles of Fe3+
moles of SCN
Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa-
tion (13) and the results of Steps 1 and 2.
moles of Fe3+
moles of SCN
9
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