Question

If $E_{Cl{O}_3^{-}/Cl{O}_4^{-}}^0=-0.36V\&E_{Cl{O}_3^{-}/Cl{O}_2^{-}}^0=0.33Vat300K.$ The equilibrium concentration of perchlorate ion $\left(Cl{O}_4^{-}\right)$ which was initially $1.0M$ in $Cl{O}_3^{-}$ when the reaction starts to attain the equilibrium,
$2Cl{O}_3^{-}\rightleftharpoons Cl{O}_2^{-}+Cl{O}_4^{-}$
Given : $Antilog(0.509)=3.329$

• A. $0.0236M$
• B. $0.0190M$
• C. $0.123M$
• D. $0.191M$

Answer 1

Answer: (D)