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28 Sep 2019
Consider thefollowing reaction:
Fe3+(aq) + SCN-(aq) FeSCN2+(aq)
A 5.0mL volume of 0.0200 M Fe(NO3)3 is mixed with 5.0 mL of 0.00200 MNaSCN; the blood-red [FeSCN2+] ion forms and an equilibrium isestablished between reactants and products. The molar concentrationof [FeSCN2+] measured spectrophotochemically is determined to be7.0 x 10-4 mol/L at equilibrium. Calculate Kc.
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Consider thefollowing reaction:
Fe3+(aq) + SCN-(aq) FeSCN2+(aq)
A 5.0mL volume of 0.0200 M Fe(NO3)3 is mixed with 5.0 mL of 0.00200 MNaSCN; the blood-red [FeSCN2+] ion forms and an equilibrium isestablished between reactants and products. The molar concentrationof [FeSCN2+] measured spectrophotochemically is determined to be7.0 x 10-4 mol/L at equilibrium. Calculate Kc.
Pleaseshow steps! Thanks
Jean KeelingLv2
28 Sep 2019
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