Consider the reaction represented by the equation: Fe3+(aq) + SCN-(aq) <====> FeSCN2+(aq) ddddd §Trial #1: 6.00...

Consider the reaction represented by the equation:

Fe3+(aq) + SCN-(aq) <====> FeSCN2+(aq) ddddd

§Trial #1:

6.00 M Fe3+(aq) and 10.0 M SCN-(aq) are mixed at a certain temperature and at equilibrium the concentration of FeSCN2+(aq) is 4.00 M.

What is the value for the equilibrium constant for this reaction?

k=0.333

§Trial #2:

Initial: 10.0 M Fe3+(aq) and 8.00 M SCN−(aq) (same temperature as Trial #1)

Equilibrium: ? M FeSCN2+(aq)

answer 5.00 M FeSCN2+

how can I solve trial #2??

Expert Solution

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queen_honey_blossom answered 2 years ago

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