1. What is Standard Cell Potential? 2. Explain what is meant by standard, and what information...
1. What is Standard Cell Potential?
2. Explain what is meant by standard, and what information is needed to calculate standard cell potential.
3. What is an example of a specific of a voltaic cell and calculate its standard cell potential showing all the work.
Homework Answers
1) The term standard represent a standard condition i.e. Temperature = 25oC. Pressure = 1 atm and concentration = 1 M or moles /L
Thus, cell potential of a cell (electrochemical cell) measured at Temperature = 25oCm, Pressure = 1 atm and concentration = 1 M or moles /L is called as standard cell potential.
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1. What is Standard Cell Potential?
2. Explain what is meant by standard, and what
information...
1) Explain what is meant by a good being "excludable."? 2) Explain what is meant by...
1) Explain what is meant by a good being "excludable."? 2) Explain what is meant by a good being "rival in consumption."? 3) Define and give an example of a public good. Is it likely that the private market provide this good on its own? Explain. 4) Define and give an example of a common resource. Without government intervention, will people use this good too much or too little? Why?
Calculate the theoretical cell potential (E°) of a galvanic cell under standard conditions made up of...
Calculate the theoretical cell potential (E°) of a galvanic cell
under standard conditions made up of copper and magnesium (see Part
II and Table 1 for more information).
PARTIL Creating and Testing Voltaic Cells Introduction and Background for the Voltaic Cells A galvanic cell (sometimes more appropriately called a voltaic cell) consists of two half-cells joined by a salt bridge that allow ions to pass between the two sides in order to maintain electroneutrality. Each half-cell contains the Components of...
how do I solve this? 1. Use the Nernst equation to calculate the standard cell potential...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
6 pts Question 7 (25) The standard cell potential (Eºcell) of voltaic cell is +1.10 V....
6 pts Question 7 (25) The standard cell potential (Eºcell) of voltaic cell is +1.10 V. Calculate the value of AGⓇ (kJ/mol) for the voltaic cell if 2 electrons are transferred between two half cells. -388 -212 +388 -24.3 +212
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) +...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
26: Voltaic Cell Diagram, Cell Potential, free-energy, K Time Left:0:14:34 Rashad Reed: Attempt 1 The following...
26: Voltaic Cell Diagram, Cell Potential, free-energy, K Time Left:0:14:34 Rashad Reed: Attempt 1 The following reaction is occurring in an voltaic cell at 25 °C Mn (s) + Br2 (1) ► Mn2+ (aq) + 2 Br(aq) The following are the standard reduction potentials: Mn2+ (aq) + 2e + Mn (5) E' = -1.18 V Br2 (1) + 2 e + 2 Br- (aq) E = 1.07 V On the paper you will submit, sketch the voltaic cell making sure...
2. Calculate the standard cell potential for each of the following redox reactions, and then predict...
2. Calculate the standard cell potential for each of the following redox reactions, and then predict whether each will occur spontaneously as written. a. Sr(s) + Fe2+(aq) → Sr2+ (aq) + Fe(s) b. 2Cr(s) + 3Cd2+ (aq) → 2Cr3+ (aq) + 3Cd(s) 3. Calculate the standard cell potential, Eºcell, for each of the voltaic cells in Part II of the experiment. a. Zn(s) | Zn2+ (aq, 1.0 M) || Cu2+ (aq, 1.0 M) Cu(s) b. Zn(s) | Zn2+(aq, 1.0 M)...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given half-reactions? Reduction Half-Reaction Ered (V) Anode -0.41 Fe2+ (aq) + 2e Fe(s) Cl2 (8) +20 +2 (aq) Cathode 1.36
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+ (aq) Cu(s) + Zn²+ (aq) E cell 1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn?' (aq) and 0.1701 M solution of Cu?+ (aq) at 441.2 K?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+...
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
Calculate the theoretical cell potential (E°) of a galvanic cell
under standard conditions made up of copper and magnesium (see Part
II and Table 1 for more information).
PARTIL Creating and Testing Voltaic Cells Introduction and Background for the Voltaic Cells A galvanic cell (sometimes more appropriately called a voltaic cell) consists of two half-cells joined by a salt bridge that allow ions to pass between the two sides in order to maintain electroneutrality. Each half-cell contains the Components of...
how
do I solve this?
1. Use the Nernst equation to calculate the standard cell potential for a voltaic cell of a Sn electrode in 0.10M Sn2(a) in one half-cell and Al in 0.10M AP) in the other. (EPe Eaode- Emode 1.52 V, Show your work. Hint: Check E values of the reduction haif reactions. Write the one with more negative E as oxidation half reaction (change the sign); ensure that equal number of electrons are exchanged ie. electrons cancel,...
6 pts Question 7 (25) The standard cell potential (Eºcell) of voltaic cell is +1.10 V. Calculate the value of AGⓇ (kJ/mol) for the voltaic cell if 2 electrons are transferred between two half cells. -388 -212 +388 -24.3 +212
Consider the reaction corresponding to a voltaic cell and its standard cell potential. cell Zn(s) + Cu2+ (aq) + Cu(s) + Zn2+ (aq) E = 1.1032 V As What is the cell potential for a cell with a 2.573 M solution of Zn²+ (aq) and 0.1055 M solution of Cu²+ (aq) at 432.4 K?
26: Voltaic Cell Diagram, Cell Potential, free-energy, K Time Left:0:14:34 Rashad Reed: Attempt 1 The following reaction is occurring in an voltaic cell at 25 °C Mn (s) + Br2 (1) ► Mn2+ (aq) + 2 Br(aq) The following are the standard reduction potentials: Mn2+ (aq) + 2e + Mn (5) E' = -1.18 V Br2 (1) + 2 e + 2 Br- (aq) E = 1.07 V On the paper you will submit, sketch the voltaic cell making sure...
2. Calculate the standard cell potential for each of the following redox reactions, and then predict whether each will occur spontaneously as written. a. Sr(s) + Fe2+(aq) → Sr2+ (aq) + Fe(s) b. 2Cr(s) + 3Cd2+ (aq) → 2Cr3+ (aq) + 3Cd(s) 3. Calculate the standard cell potential, Eºcell, for each of the voltaic cells in Part II of the experiment. a. Zn(s) | Zn2+ (aq, 1.0 M) || Cu2+ (aq, 1.0 M) Cu(s) b. Zn(s) | Zn2+(aq, 1.0 M)...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given half-reactions? Reduction Half-Reaction Ered (V) Anode -0.41 Fe2+ (aq) + 2e Fe(s) Cl2 (8) +20 +2 (aq) Cathode 1.36
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu?+ (aq) Cu(s) + Zn²+ (aq) E cell 1.1032 V What is the cell potential for a cell with a 2.344 M solution of Zn?' (aq) and 0.1701 M solution of Cu?+ (aq) at 441.2 K?
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s) + Cu2+ (aq) Cu(s) + Zn2+ (aq) ЕО cell = 1.1032 V What is the cell potential for a cell with a 2.440 M solution of Zn2+ (aq) and 0.1636 M solution of Cu²+ (aq) at 439.5 K?
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