HClO(aq) = Cl2 (aq) Eo = + 1.611V
MnO4-1(aq) = MnO2(s) Eo = + 1.679V
In...
HClO(aq) = Cl2 (aq) Eo = + 1.611V
MnO4-1(aq) = MnO2(s) Eo = + 1.679V
In a particular cell, Ecell is measured to be +0.038v
when the pH in both half-cells is 4.00 and [Cl2] = 0.20 M, [HClO] =
0.10 M. What is [MnO4-1] in the solution?
Balance the following redox equation in basic conditions:
Ag(s) + MnO4⁻(aq) ⟶
MnO2(s) + Ag+(aq)
What is the stochiometric coefficient for H2O in the
balanced equation?
Consider the following reactions. reaction
MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution
Balance each equation under the specified conditions
Write unbalanced half-reactions for the following net ionic
equations.
Part A MnO4−(aq)+IO3−(aq)→MnO2(s)+IO4−(aq) Express your answers
as chemical expressions separated by a comma. Enter the reduction
half-reaction first. Identify all of the phases in your answer.
Part B NO3−(aq)+SO2(aq)→SO42−(aq)+NO2(g) Express your answers as
chemical expressions separated by a comma. Enter the reduction
half-reaction first. Identify all of the phases in your answer.
The value of the equilibrium constant for the electrochemical
reaction
MnO4–(aq) +
2H+(aq) + ½Cl2(g)
⇌Mn2+(aq)+
ClO3–(aq)
+H2O(aq)
is 5.88 x10–5. What is the value of the equilibrium
constant for the reverse reaction?
An MnO2(s) /Mn2+(aq) electrode in which the pH is 10.18 is
prepared. Part A Find the [Mn2+] necessary to lower the potential
of the half-cell to 0.00 V (at 25 ∘C). Express your answer using
two significant figures. [Mn2+] =