Step 3 How many moles of Fe* and SCN" remain in solution at equilibrium? Use the results of Steps 1 and 2, noting that moles SCN¯ at equilibrium = original moles SCN" – (2 × moles Fe(SCN), *). moles Fe"; _moles SCN" Step 4 What are the concentrations of Fe". SCN", and Fe(SCN),* at equilibrium? (Use Eq. 3 and the results of Step 3.) [Fe*] = _M; [SCN¯] = . _M: [Fe(SCN),*] = Step 5 Calculate K̟ based on the assumption that the altermate reaction occurs. (Use the answer to Part 2a.)

Step 3 How many moles of Fe* and SCN" remain in solution at equilibrium? Use the results of Steps 1 and 2, noting that moles SCN¯ at equilibrium = original moles SCN" – (2 × moles Fe(SCN), ). moles Fe"; _moles SCN" Step 4 What are the concentrations of Fe". SCN", and Fe(SCN), at equilibrium? (Use Eq. 3 and the results of Step 3.) [Fe] = _M; [SCN¯] = . _M: [Fe(SCN),] = Step 5 Calculate K̟ based on the assumption that the altermate reaction occurs. (Use the answer to Part 2a.)

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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Question

Step 3 How many moles of Fe* and SCN" remain in solution at equilibrium? Use the results of Steps 1
and 2, noting that moles SCN¯ at equilibrium = original moles SCN" – (2 × moles Fe(SCN), *).
moles Fe";
_moles SCN"
Step 4 What are the concentrations of Fe". SCN", and Fe(SCN),* at equilibrium? (Use Eq. 3 and the
results of Step 3.)
[Fe*] =
_M; [SCN¯] = .
_M: [Fe(SCN),*] =
Step 5 Calculate K̟ based on the assumption that the altermate reaction occurs. (Use the answer to Part 2a.)

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