How to Determine Cell Reaction and Ksp of CuBr?

AI Thread Summary
The discussion focuses on determining the overall cell reaction and calculating the solubility product constant (Ksp) of CuBr at 298K, given the electrochemical cell setup. Participants are encouraged to simplify the reaction involving CuBr into its ionic components, specifically Cu+ and Br-. Additionally, the impact of increasing the pressure of H2 from 1 atm to 2 atm on the electromotive force (EMF) is questioned, with references to Le Chatelier's principle for understanding the effects of pressure changes on the equilibrium. Clarification on how to approach these calculations and the underlying principles is sought. Understanding these concepts is essential for solving the homework problem effectively.
lioric
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Homework Statement



Pt l H2 (1atm) l HBr (1x10-4M) ll CuBr l Cu = 0.599 V at 298K

i) determine the overall cell reation and calculate the Ksp of CuBr at 298K
ii) What would be the effect on EMF if pressure of H2 increases from 1atm to 2atm. Why?


Homework Equations



CuBr = Cu+ x Br-

The Attempt at a Solution


I don't know how to simplify this equation to ions
And can someone explain what the pressure change would do? Do i have to think about the La chatlear's principles?
 
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Start writing two separate half cell reactions.
 
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