2. A student mixes 5.0 mL of 2.00 x 10³ M Fe(NO3)3 with 3.0 mL of 2.00 x 10³ M KSCN and2.0 mL of water. She finds that the equilibrium concentration of FeSCN²+ is 4.03 x 104 M.Use an ICE table to determine the equilibrium concentrations of each chemical and theequilibrium constant for the reaction.

Answered: 2. A student mixes 5.0 mL of 2.00 x 10³…

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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2. A student mixes 5.0 mL of 2.00 x 10³ M Fe(NO3)3 with 3.0 mL of 2.00 x 10³ M KSCN and
2.0 mL of water. She finds that the equilibrium concentration of FeSCN²+ is 4.03 x 104 M.
Use an ICE table to determine the equilibrium concentrations of each chemical and the
equilibrium constant for the reaction.

Expert Solution

Step 1: Equilibrium constant

When both the conversion of reactants to products and products to reactants are feasible in a system, the system will eventually reach a state at which both processes occur at the same rate. This state is called the equilibrium state.

Consider the following general equation-

$pP plus qQ left right double arrow rR plus sS$

The equilibrium constant (K) for the given reaction is shown as follows-

$K equals fraction numerator left square bracket S right square bracket to the power of s open square brackets R close square brackets to the power of r over denominator open square brackets P close square brackets to the power of p open square brackets Q close square brackets to the power of q end fraction$

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