If the reduction reaction has a reduction potential of 0.1 V, and the oxidation reaction has...
If the reduction reaction has a reduction potential of 0.1 V, and the oxidation reaction has a reduction potential of -0.4V, and 2 electrons were transfered, what is the value of delta G expressed in terms of F?
The simplified Nernst equation is
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If the reduction reaction has a reduction potential of 0.1 V,
and the oxidation reaction has...
The cell potential of a redox reaction occurring in an electrochemical cell under any set of...
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
28. (8) An oxidation-reduction reaction in which 3 electrons are transferred has ΔΟ. +18.55 kl at...
28. (8) An oxidation-reduction reaction in which 3 electrons are transferred has ΔΟ. +18.55 kl at 25 °C. What is the value of E°? a. +0.192 V b. -0.064 V c. -0.192 V d. -0.577 V e. +0.064 V
The free energy change for an oxidation-reduction reaction occurring at constant temperature and pressure is given...
The free energy change for an oxidation-reduction reaction occurring at constant temperature and pressure is given by AGnFE where n is the moles of electrons transferred in the reaction, E is the cell potential of the reaction, and F is Faraday's constant. Use this relationship to answer the problem below In one half-cell of a voltaic cell, the following reaction occurs: Be(s) → Be2+(aq) + 2 e. In the other half-cell of the voltaic cell, the following reaction occurs: 2...
Below are the paired reduction reactions for chemolithotrophic denitrification: these organisms are using nitrate as an...
Below are the paired reduction reactions for chemolithotrophic denitrification: these organisms are using nitrate as an electron accepter and are using hydrogen gas as a source of energy and electrons. 2NO3- + 10e- -> N2 (+0.74 volts) 2H+ + 2e- -> H2 (-0.42 volts) Using the information given, calculate the ΔE for this reaction, balance the full reaction to determine n, the number of electrons transfered when 97 molecules of H2 are oxidized. Finally, use the simplified Nernst Equation ΔG...
Below are the paired reduction reactions for chemolithotrophic denitrification: theseorganisms are using nitrate as an electron...
Below are the paired reduction reactions for chemolithotrophic denitrification: theseorganisms are using nitrate as an electron accepter and are using hydrogen gas as a source of energy and electrons. 2NO3- + 10e- -> N2 (+0.74 volts) 2H+ + 2e- -> H2 (-0.42 volts) Using the information given, calculate the ΔE for this reaction, balance the full reaction to determine n, the number of electrons transfered when 53 molecules of H2 are oxidized. Finally, use the simplified Nernst Equation ΔG =...
Below are the reduction half reactions for chemolithoautotrophic nitrification, where ammonia is a source of electrons...
Below are the reduction half reactions for chemolithoautotrophic nitrification, where ammonia is a source of electrons and energy and oxygen is the terminal electron acceptor. NO2- + 6e- -> NH4+ (-0.41 volts) O2 + 4e- -> 2H2O (+0.82 volts) Using the information given, calculate the ΔE for this reaction, balance the full reaction to determine the n, the number of electrons transfered when 3 molecules of NH4+ are oxidized. Finally, use the simplified Nernst Equation ΔG = -nFΔE, where F...
(a) What is the reduction potential of the half reaction in which V2+ is reduced to...
(a) What is the reduction potential of the half reaction in
which V2+ is reduced to V?
(b) Give the balanced half equation and accompanying E° value
for the reduction half-reaction with the largest (most positive) E°
value that involves a pair of species indicated in the Frost
diagram.
(c) Indicate which species, if any, will undergo
disproportionation.
(d) Give the balanced reduction half-equation and accompanying
E° value for the reduction of VO2+ to V2+.
(e) In the Pourbaix diagram...
help when an electrochemical process - oxidation and reduction - Occurs - the contraction " is...
help
when an electrochemical process - oxidation and reduction - Occurs - the contraction " is often used to describe it. 2. Oxidation is the circle one) loss gain of electrons by an atom, ion, or molecule. 3. Reduction is the circle one) loss gain of electrons by an atom, ion, or molecule. 4. What is the name of the electrode at which reduction occurs?ge 5. What is the name of the electrode at which oxidation occurs? 6. True or...
1. 2. 3. Balancing Oxidation-Reduction Reactions 1. Assign oxidation numbers. 2. Separate into oxidation and reduction...
1. 2. 3.
Balancing Oxidation-Reduction Reactions 1. Assign oxidation numbers. 2. Separate into oxidation and reduction half reactions. 3. Balance each half reaction using the following steps: a. Balance all elements except oxygen or hydrogen. b. Balance oxygen by adding H20. c. Balance hydrogen by adding H*. d. Balance charge by adding electrons: Electrons go on the RIGHT (product side) for OXIDATION reactions. Electrons go on the LEFT (reactant side) for REDUCTION reactions. e. In BASIC solution, do this additional...
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
28. (8) An oxidation-reduction reaction in which 3 electrons are transferred has ΔΟ. +18.55 kl at 25 °C. What is the value of E°? a. +0.192 V b. -0.064 V c. -0.192 V d. -0.577 V e. +0.064 V
The free energy change for an oxidation-reduction reaction occurring at constant temperature and pressure is given by AGnFE where n is the moles of electrons transferred in the reaction, E is the cell potential of the reaction, and F is Faraday's constant. Use this relationship to answer the problem below In one half-cell of a voltaic cell, the following reaction occurs: Be(s) → Be2+(aq) + 2 e. In the other half-cell of the voltaic cell, the following reaction occurs: 2...
(a) What is the reduction potential of the half reaction in
which V2+ is reduced to V?
(b) Give the balanced half equation and accompanying E° value
for the reduction half-reaction with the largest (most positive) E°
value that involves a pair of species indicated in the Frost
diagram.
(c) Indicate which species, if any, will undergo
disproportionation.
(d) Give the balanced reduction half-equation and accompanying
E° value for the reduction of VO2+ to V2+.
(e) In the Pourbaix diagram...
help
when an electrochemical process - oxidation and reduction - Occurs - the contraction " is often used to describe it. 2. Oxidation is the circle one) loss gain of electrons by an atom, ion, or molecule. 3. Reduction is the circle one) loss gain of electrons by an atom, ion, or molecule. 4. What is the name of the electrode at which reduction occurs?ge 5. What is the name of the electrode at which oxidation occurs? 6. True or...
1. 2. 3.
Balancing Oxidation-Reduction Reactions 1. Assign oxidation numbers. 2. Separate into oxidation and reduction half reactions. 3. Balance each half reaction using the following steps: a. Balance all elements except oxygen or hydrogen. b. Balance oxygen by adding H20. c. Balance hydrogen by adding H*. d. Balance charge by adding electrons: Electrons go on the RIGHT (product side) for OXIDATION reactions. Electrons go on the LEFT (reactant side) for REDUCTION reactions. e. In BASIC solution, do this additional...
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