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cliffordlim
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Homework Statement
Fe2+and Cr2O72- react as follows: 6Fe2+ + Cr2O7 2− + 14H + >>> 6Fe3+ + 2Cr3+ + 7H2O.
The equilibrium constant for the reaction is 1×10^57. Calculate the equilibrium concentrations
of the iron and chromium species if 10 mL each of 0.02M K2Cr2O7 in 1.14M HCl and 0.12M FeSO4
in 1.14M HCl are reacted.
Homework Equations
The Attempt at a Solution
https://physicsforums-bernhardtmediall.netdna-ssl.com/data/attachments/97/97696-2f7ec586395970f64d734682baf6f166.jpg
This is the solution provided . I still don't understand as Cr3+ is 0.02M in the equation as the question give is K2Cr2O7 is 0.02M > does it mean 0.02M of Cr2O72- ? Same goes to iron .
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