Study this chemical reaction: 2Fe (s) + 3PbNO32 (aq) ? 3Pb (s) +
2FeNO33 (aq) Then,...
Study this chemical reaction: 2Fe (s) + 3PbNO32 (aq) ? 3Pb (s) +
2FeNO33 (aq) Then, write balanced half-reactions describing the
oxidation and reduction that happen in this reaction. ?
Study this chemical reaction:
2Fe + 3I2---> 2FeI3
Then, write balanced half-reactions describing the oxidation and
reduction that happen in this reaction.
oxidation:
reduction:
A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq)
Calculate the cell potential at 25 ∘C under each of the following
conditions.
1.) [Fe3+]= 1.1×10−3 M ; [Mg2+]= 2.60 M
2.) [Fe3+]= 2.60 M ; [Mg2+]= 1.1×10−3 M
A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq)
Calculate the cell potential at 25 ∘C under each of the following
conditions
a)[Fe3+]= 1.0×10−3 M ; [Mg2+]= 2.00 M
b)[Fe3+]= 2.00 M ; [Mg2+]= 1.0×10−3 M
A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at
25 ∘C under each of the following conditions.
A) [Fe3+]= 1.9×10−3 M ; [Mg2+]=
2.80 M
B) [Fe3+]= 2.80 M ; [Mg2+]= 1.9×10−3 M
A voltaic cell employs the following redox reaction:
2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at
25 ∘C under each of the following conditions.
Part A standard conditions
Part B [Fe3+]=1.9×10−3
M
;
[Mg2+]=1.80
M
Part
C [Fe3+]=1.80
M
;
[Mg2+]=1.9×10−3
M
For the following chemical reaction:
Ba2+(aq) + 2OH-(aq) +
H2O2(aq) +
2ClO2(aq) -->
Ba(ClO2)2(s) +
2H2O(l) + O2(g)
a) Assign oxidation numbers to each element.
b) State the elements undergoing oxidation.
c) State the elements undergoing reduction.
d) State the oxidizing agent.
e) State the reducing agent.
f) State the total number of electrons being transferred during
the reaction.
Consider the balanced chemical reaction Cu(s) + 2AgNO3(aq) a
2Ag(s) + Cu(NO3)2(aq)
a) Write the Complete Ionic Equation:
b) Write the Net Ionic Equation:
c) Assign oxidation numbers to all of atoms/ions in the
reaction:
Cu _____ Ag _____ NO3_____ a Ag _____ Cu _____ NO3 _____
d) Which atom/ion is being oxidized in this reaction?
e) Which atom/ion is being reduced in this reaction?
Lab Reaction Rate and order of
a Chemical Reaction
H3AsO3 (aq) +
I3- (aq) + H2O (l) →
HAsO42- (aq) + 3 I- (aq) +
4H+ (aq)
The data has been collected and
pre-lab completed. Need help with the results.
Results
Laboratory temperature: 25°C
DATA TABLE 1:
Experiment
[IO3]0
[H+]0
[H3AsO3]0
[I]0
1
.005
.00001
.0015
.05
2
.01
.00001
.0015
.05
3
.005
.00001
.0015
.1
4
.005
.00002
.0015
.05
DATA TABLE 2:
Experiment
Δt (s)
Δ[IO3-]...
Calculate the equilibrium constant for each of the reactions at
25 ∘C .
A.)
2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
B.)
O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq)
C.)
Br2(l)+2I−(aq)→2Br−(aq)+I2(s)