The standard cell potential for the reaction in a fuel cell that uses the reaction CH 4(g) +2O 2(g) → CO 2(g) +2H 2 O (g) is to be calculated. Introduction: The cell potential of a certain electrochemical cell states how much voltage generates between two half cells of that electrochemical cell. We can denote the cell potential as E 0 . On the other hand, the free energy change or Δ G 0 is a thermodynamic quantity that describes the internal energy of the electrochemical cell which is available to generate electricity. There is a relationship between cell potential and free energy change as follows: Δ G 0 = − n F E 0 Where, n is the number of moles of electrons that transfer during the reaction while F is the Faraday Constant. We can calculate the standard cell potential using the standard free energies of formation ( Δ G 0 f ) of reactants and products of a given reaction. The equation for this calculation is Δ G 0 = [ Δ G 0 f ( R e a c t a n t s ) ] − [ Δ G 0 f ( P r o d u c t s ) ]
The standard cell potential for the reaction in a fuel cell that uses the reaction CH 4(g) +2O 2(g) → CO 2(g) +2H 2 O (g) is to be calculated. Introduction: The cell potential of a certain electrochemical cell states how much voltage generates between two half cells of that electrochemical cell. We can denote the cell potential as E 0 . On the other hand, the free energy change or Δ G 0 is a thermodynamic quantity that describes the internal energy of the electrochemical cell which is available to generate electricity. There is a relationship between cell potential and free energy change as follows: Δ G 0 = − n F E 0 Where, n is the number of moles of electrons that transfer during the reaction while F is the Faraday Constant. We can calculate the standard cell potential using the standard free energies of formation ( Δ G 0 f ) of reactants and products of a given reaction. The equation for this calculation is Δ G 0 = [ Δ G 0 f ( R e a c t a n t s ) ] − [ Δ G 0 f ( P r o d u c t s ) ]
Solution Summary: The author explains how to calculate the standard cell potential for the reaction in a fuel cell.
Definition Definition Study of chemical reactions that result in the production of electrical energy. Electrochemistry focuses particularly on how chemical energy is converted into electrical energy and vice-versa. This energy is used in various kinds of cells, batteries, and appliances. Most electrochemical reactions involve oxidation and reduction.
Chapter 19, Problem 19.73SP
Interpretation Introduction
Interpretation:
The standard cell potential for the reaction in a fuel cell that uses the reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) is to be calculated.
Introduction:
The cell potential of a certain electrochemical cell states how much voltage generates between two half cells of that electrochemical cell. We can denote the cell potential as E0. On the other hand, the free energy change or ΔG0 is a thermodynamic quantity that describes the internal energy of the electrochemical cell which is available to generate electricity. There is a relationship between cell potential and free energy change as follows:
ΔG0=−nFE0
Where, n is the number of moles of electrons that transfer during the reaction while F is the Faraday Constant.
We can calculate the standard cell potential using the standard free energies of formation ( ΔG0f ) of reactants and products of a given reaction. The equation for this calculation is
A voltaic cell was build upon the following redox reaction:
4 Ag (s) + O2 (g) + 4 H+ (aq) →4 Ag (s) + 2 H2O (l)
Under standard condition, the cell produces 0.43 V voltage. What is the ΔGo for this reaction? Is this reaction spontaneous or non-spontaneous?
A certain metal M forms a soluble sulfate salt M,SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 22.5 mM solution of M,SO,
and the right half cell with a 4.50 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected
between them. The temperature of the apparatus is held constant at 25.0 °C.
O left
Which electrode will be positive?
O right
What voltage will the voltmeter show? Assume its positive lead is connected to the
positive electrode.
Be sure your answer has a unit symbol, if necessary, and round it to 2 significant
digits.
A certain metal M forms a soluble sulfate salt M, SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution
of M, SO, and the right half cell with a 2.00 mM solution of the same substance. Electrodes made of M are dipped into both solutions and
a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C.
left
Which electrode will be positive?
right
What voltage will the voltmeter show? Assume its positive lead is connected to the
positive electrode.
Be sure your answer has a unit symbol, if necessary, and round it to 2 significant
digits.
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