Question

1. When the following equation is balanced properly under basic
conditions, what are the coefficients of the species shown?

**__N _{2}H_{4}** +
__

Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of ___. (Enter 0 for neither.)

Which

2. Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction:

**2****Cr ^{3+}**

Answer: ___ kJ

K for this reaction would be __greater or less__ than one.

Answer #1

A) When the following equation is balanced properly under acidic
conditions, what are the coefficients of the species shown?
_Fe2++ _PbO2
---> _Fe3++
_Pb2+
Water appears in the balanced equation as a ____ (reactant,
product, neither) with a coefficient of .
Which element is reduced? ___
B) When the following equation is balanced properly under acidic
conditions, what are the coefficients of the species shown?
_Cr2++
_Fe2+--->
_Cr3++ _Fe
Water appears in the balanced equation as a ____ (reactant,
product,...

When the following equation is balanced properly under acidic
conditions, what are the coefficients of the species shown?
Mn2+ + NO3- MnO2 + HNO2
Water appears in the balanced equation as a (reactant, product,
neither) with a coefficient of . (Enter 0 for neither.)
How many electrons are transferred in this reaction?

When the following equation is balanced properly under acidic
conditions, what are the coefficients of the species shown?
_____ HNO2 + _____
NiO2
----->____NO3- + ____
Ni2+
Water appears in the balanced equation as a _____ (reactant,
product, neither) with a coefficient of _____. (Enter 0 for
neither.)
How many electrons are transferred in this reaction? ______

When the following equation is balanced properly under acidic
conditions, what are the coefficients of the species shown?
BrO3- + ClO2 Br- + ClO3-
Water appears in the balanced equation as a (reactant,
product, neither) with a coefficient of . (Enter 0 for
neither.)
How many electrons are transferred in this reaction?

When the following skeletal equation is balanced under basic
conditions, what are the coefficients of the species shown?
F-+ HPbO2-
-----> F2+ Pb
Water appears in the balanced equation as a _____(reactant,
product, neither) with a coefficient of_____ . (Enter 0 for
neither.)
Which species is the reducing
agent?_____

1) The free energy change for the following reaction at 25 °C,
when [Pb2+] = 1.18 M
and [Cd2+] =
7.90×10-3 M, is -65.9
kJ:
Pb2+(1.18 M) +
Cd(s)>
Pb(s) +
Cd2+(7.90×10-3
M) ΔG = -65.9 kJ
What is the cell potential for the reaction as written under these
conditions?
Answer: ___V
Would this reaction be spontaneous in the forward or the reverse
direction?
2) Use the standard reduction potentials located in the 'Tables'
linked above to calculate the standard...

Balance the reaction between Ag and
Br2 to form
Br- and
Ag2O in basic solution. When you have
balanced the equation using the smallest integers possible, enter
the coefficients of the species shown.
___Ag + ___Br2
----> ___Br- +
___Ag2O
Water appears in the balanced equation as a ____(reactant, product,
neither) with a coefficient of ___. (Enter 0 for neither.)
How many electrons are transferred in this reaction? ____

What are the coefficients for the following reaction when it is
properly balanced? What are the coefficients for the following
reaction when it is properly balanced?
_HCl+_Mg +MgCl2+_H2
2, 1, 1, 1
2, 1, 2, 2
1, 2, 1/2, 1
1, 1, 1, 2

Balance the half-reaction below for basic solution:
NH4+(aq) → N2H4(aq)
Which one of the following statements is correct? You should use
the smallest possible integer coefficients in the balanced
equation.
[Note that H2O(l) and OH–(aq) may have to be added
where necessary to balance the equation.]
2OH– appears on the left; this is an oxidation.
4OH– appears on the left; this is an oxidation.
2OH– appears on the right; this is a reduction.
4OH– appears on the left; this is...

Enter electrons as
e-.
Use smallest possible
integer coefficients.
If a box is not needed, leave it
blank.
Use the table 'Standard Reduction Potentials' located in the
'Tables', to predict if a reaction will occur when
Fe metal is put into a 1M aqueous
Cd2+ solution.
If a reaction will occur, write a balanced net ionic equation for
the reaction. If no reaction will occur, leave all boxes
blank.
___ + ___ ------> ___+ ___
Use a table of Standard...

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