What is the redox of: ClO- (aq) + IO3- (aq) → ClO3- (aq) + I2 (s)...

What is the redox of:

ClO^- (aq) + IO₃^- (aq) → ClO₃^- (aq) + I₂ (s) [A]

Expert Solution

queen_honey_blossom answered 2 years ago

Balance the following redox reaction occurring in basic solution. I−(aq)+MnO−4(aq)→I2(aq)+MnO2(s)

Consider the following unbalanced redox reaction occurring in acidic solution: H2SO3 (aq) + IO3-(aq) → SO42-(aq)...

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^-...

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) +...

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) +...

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...

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?

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq)...

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq) +2e- <---> 2I-(aq) E0 = 0.620 V I3-(aq) + 2e- <---> 3I-(aq) E0 = 0.535 V a) Calculate the equilibrium constant for I2(aq) + I-(aq) <---> I3-(aq) b) Calculate the equilibrium constant for I2(s) + I-(aq) <---> I3-(aq) c) Calculate the solubility (g/L) of I2(s) in water.

Balance the following redox equation in basic conditions: Ag(s) + MnO4⁻(aq) ⟶ MnO2(s) + Ag+(aq) What...

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?

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)...

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.

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance...

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance each equation under the specified conditions

Question

What is the redox of: ClO- (aq) + IO3- (aq) → ClO3- (aq) + I2 (s)...

Solutions

Expert Solution

Related Solutions

Balance the following redox reaction occurring in basic solution. I−(aq)+MnO−4(aq)→I2(aq)+MnO2(s)

Consider the following unbalanced redox reaction occurring in acidic solution: H2SO3 (aq) + IO3-(aq) → SO42-(aq)...

1.Balance the redox reaction first ( it is in basic medium) ClO^-(aq) + CrO2^-(aq) -----> Cl^-...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

when the following redox reaction is balanced Pb(s) + SnCl4 (aq) -> Sn(s) +PbCl2 (aq) what...

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq)...

Balance the following redox equation in basic conditions: Ag(s) + MnO4⁻(aq) ⟶ MnO2(s) + Ag+(aq) What...

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)...

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance...