Question

Complete and balance the equation where Cl2 reacts with Ag+ in an acidic solution to yield AgCl(s) and ClO3-.

Answer #1

**Cl2 ---> Cl03-**

**first balance atoms other than O and H**

**Cl2 --> 2 Cl03-**

**now balance O atoms using H20**

**Cl2 + 6 H20 --> 2 Cl03-**

**now balance H atoms using H+**

**Cl2 + 6 H20 ---> 2 Cl03- + 12 H+**

**now balance charge using e-**

**Cl2 + 6 H20 ---> 2 Cl03- + 12 H+ + 10e-**

**now**

**consider the reaction**

**Cl2 + Ag+ ---> AgCl**

**first balance the atoms other than O and H**

**Cl2 + 2Ag+ ---> 2 AgCl**

**there are no O and H atoms**

**so balance charge using e-**

**Cl2 + 2 Ag+ + 2e- ---> 2 AgCl**

**now**

**write both the equations so that e- are
equal**

**so**

**Cl2 + 6 H20 ---> 2 Cl03- + 12 H+ + 10e-**

**5Cl2 + 10 Ag+ + 10e- ---> 10 AgCl**

**cancel out the electrons**

**we get**

**6 Cl2 + 6H20 + 10Ag+ ---> 2 Cl03- + 12H+ + 10
AgCl**

**3 Cl2 + 3H20 + 5 Ag+ --> Cl03- + 6H+ + 5
AgCl**

Balance these equations for redox reactions occurring in acidic
solution.
VO43−+Fe2+→VO2++Fe3+
Balance these equations for redox reactions in basic
solution.
MnO2(s)+ClO3−→MnO4−+Cl−

Balance this net ionic equation: Ag((NH3)2)^+) + (H^+) + (Cl^-)
---> AgCl(s) + NH3

Complete and balance this equation for a reaction in acidic
medium using smallest whole #'s.
Reaction: As2O3 + NO-3----> H3AsO4 + NO (split into 1/2
reactions first)

Cl2(aq) + OF- (aq) --> ClO3- + F- (aq)
a) use the half reaction method to balance in acidic
solution.
b) use the half reaction method to balance in basici
solution.

Part A Complete and balance the following equation:
NO?2(aq)+Cr2O2?7(aq)?Cr3+(aq)+NO?3(aq) (acidic solution)
Express your answer as a chemical equation. Identify all of the phases in your
answer.
Identify the oxidizing and reducing agents in equation
above.
Express your answers as chemical expressions separated by a
comma
Part C
Complete and balance the following equation:
BrO?3(aq)+N2H4(aq)?Br2(l)+N2(g)
(acidic solution)
Express your answer as a chemical equation. Identify all of the
phases in your answer.
Part D
Identify the oxidizing and reducing agents in...

Match the redox equation with the number and location of water
molecules that appear in the equation when it is correctly
balanced.
-A.B.C.D.E.F.G.H.I.J.
Fe+2 (aq) + H2O2 (aq) -->
Fe+3 (aq) in acidic solution
-A.B.C.D.E.F.G.H.I.J.
Cl2 (aq) --> ClO3- (aq) +
Cl- in acidic solution
-A.B.C.D.E.F.G.H.I.J.
Sn (s) + NO3- (aq) --> Sn+2
(aq) + NO (g) in acidic solution
-A.B.C.D.E.F.G.H.I.J.
Ag (s) + HS- (aq) + CrO4-2 (aq)
--> Ag2S (s) + Cr(OH)3 (s) in basic
solution
A.
3...

BALANCE THE FOLLOWING EQUATION IN ACIDIC SOLUTION. 1. Mn2+ +
IO3- MnO2 + I2

Use half-reactions to balance the following equation in acidic
solution:
Fe2+ + IO3- = Fe3+ + I2

Balance the following equation in an acidic and basic
solution.
Br-(aq)+NO3<---->NO-(g)+Br2(l)

1) sulfuric acid reacts with the ammonia according to the
equation below. It takes 32.89 mL of a 1.50 M solution of sulfuric
acid to neutralize 64.7 mL of ammonia solution. what is the molar
concentrationof the ammonia solution? H2SO4 (aq) + 2 NH3
(aq)---> (NH4)2SO4 (aq)
2) A 500.0mL solution that contains silver ion is treated with
excess sodium chloride soultion, producing a precpitate of silver
chloride that has a mass of 45.4 mg. What mass of silver ion...

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