A reaction: A (aq) + B (aq) <-----> C (aq) has a standard
free energy change of -3.05 kJ/mol at 25 C. What are the
concentrations of A, B, and C at equilibrium if, at the beginning
of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M,
respectively?
A = ? M
B= ? M
C= ? M
How would your answer above change if the reaction had a
standard free energy change of +3.05 kJ/mol?
A.)...
What is the standard Gibb’s Free Energy of the reaction graphite
| Br-(aq) | Br2(l) | |
I2(s) | I-(aq)? Is the
reaction spontaneous under standard conditions?
What is the initial cell potential of the voltaic cell
represented by Zn | Zn+2 [0.100 M) | | Ni+2
(1.50 M) | Ni ?
b. What is the cell potential when [Ni+]=0.500 M?
c. What are the metal ion concentrations when the cell potential
has fallen to 0.45 V?
4. Calculate the standard reduction potential and the standard
free energy change for each of the following oxidation-reduction
reactions:
a. Ubiquinol (QH2) + 2 Cytochrome C(Fe +3) <-------->
Ubiquinone (Q) + 2 Cytochrome C(Fe+2) + 2H+
b. Succinate + ½ O2 <--------> Fumarate + H2O
c. Explain how odd chain fatty acids can serve as gluconeogenic
precursors.
. Consider the following reduction-oxidation “skeleton”
equation,
Br2(l) = BrO3 ‒ (aq) + Br‒ (aq)
a. Write a balanced equation for the reduction-oxidation
reaction that occurs in basic solution.
b. Using your balanced equation, identify the chemical species
that is: (1) oxidized, (2) reduced, (3) the reducing agent, and (4)
the oxidizing agent.
Calculate ΔG° for the following reaction as written
Ni2+ (aq) + Sn (s) → Ni (s) + Sn2+
(aq)
given the following reduction half-reactions and standard
reduction potentials.
Sn2+ (aq) + 2 e- → Sn (s)
E° = -0.15V
Ni2+ (aq) + 2 e- → Ni (s)
E° = -0.25V
Consider the reaction NH4Cl(aq)NH3(g) + HCl(aq) The standard
free energy change for this reaction is 62.8 kJ.
The free energy change when 1.72 moles of NH4Cl(aq) react at
standard condition is____ kJ.
What is the maximum amount of useful work that the reaction of
1.72 moles of NH4Cl(aq) is capable of producing in the surroundings
under standard conditions?_______
If no work can be done, enter none. kJ
A reaction
A(aq) + B(aq) --> C(aq)
has a standard free-energy change of –3.23 kJ/mol at 25 °C. What
are the concentrations of A, B, and C at equilibrium if, at the
beginning of the reaction, their concentrations are 0.30 M, 0.40 M,
and 0 M, respectively?
Calculate the overall standard electromotive force (ΔE°') and
free energy (ΔG°') for the reaction below. Show all work. Pyruvate
+ NADH + H+ lactate + NAD+
Calculate the free-energy change of the following reaction at
352°C and standard pressure. Values in the table are at standard
pressure and 25°C.
C2H4 + 3O2 --> 2CO2 +2H2O
ΔHºf,(kJ/mol)
Sºf,
J/mol•K
ΔGºf,
kJ/mol
C2H4(g)
52.3
219.5
68.1
O2(g)
0
205.0
0
CO2(g)
-393.5
213.6
-394.4
H2O(g)
-241.8
188.7
-228.6
Reaction 1: Cu(s) + AgNO3 (aq) = CuNO3 (aq) + Ag (s)
Reaction 2: Cu (s) +AgNO3 (aq) = Cu(NO3)2 (aq) + Ag (s)
Part 1: Write the balanced net ionic equations for both of the
above reactions.
Assume that excess silver nitrate is available when answering
the remaining questions.
Part 2: Calculate the theoretical grams of silver metal that
could form from 2.568g of copper wire based upon reaction 1. (Be
sure the reaction is properly balanced.)
Part 3:...