Consider the following unbalanced redox reaction occurring in
acidic solution: H2SO3 (aq) + IO3-(aq) → SO42-(aq) + I2 (aq) a)
Balance the reaction. b) Using your table of standard reduction
potentials, calculate ΔG°rxn for this reaction.
1.Balance the redox reaction first ( it is in basic medium)
ClO^-(aq) + CrO2^-(aq) -----> Cl^- (aq) +CrO4^-2(aq)
2. A titration experiment is set up to use .185M bleach (NaOCl)
to analyze CrO2^-.If 50.0mL of the CrO2^-(aq) solution required
32.53mL of bleach to react to completion, what would you calculate
as the molarity of the CrO2^- solution?
1)What element is being oxidized in the following redox
reaction?
Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^-
1B) Balance the following redox reaction if it occurs in acidic
solution. What are the coefficients in frot of H+ and Fe3+ in the
balance reaction?
Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+
1C) determine the cell notation for the redox reaction given
below. [hint: remember sometimes inert electrodes are used.
3 Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2...
1)What element is being oxidized in the following redox
reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^-
1B) Balance the following redox reaction if it occurs in acidic
solution. What are the coefficients in frot of H+ and Fe3+ in the
balance reaction? Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn
2+
1C) determine the cell notation for the redox reaction given
below. [hint: remember sometimes inert electrodes are used. 3
Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2...
when the following redox reaction is balanced Pb(s) + SnCl4
(aq) -> Sn(s) +PbCl2 (aq) what is the coefficient in front of
the species that underwent oxidation?
Calculate E?cell for each of the following balanced
redox reactions.
A.
O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq)
B.
Br2(l)+2I?(aq)?2Br?(aq)+I2(s)
C.
PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)
D. Determine whether the reaction in part A is spontaneous as
written.
E. Determine whether the reaction in part B is spontaneous as
written.
F. Determine whether the reaction in part C is spontaneous as
written.
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