Homework Answers
Option D is not true about the junction potential. It should be directly proportional to the difference between the half cell potentials (Ered-Eox). As, the difference between the half cell potentials increases, junction potential also increases. Thus, a salt bridge is provided to maintain the electrical neutrality of the solution so that the liquid junction potential (LJP) is almostalmost equal to zero.
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Which of the following is not true about the junction potential? A. It depends on the...
The junction potential develops due to charge separation T F. The junction potential in a salt...
The junction potential develops due to charge separation T F. The junction potential in a salt bridge can be reduced somewhat if ions with similar mobilities are used inside the salt bridge. T F Junction potentials put a fundamental limit on the accuracy of direct potentiometric measurements T F The junction potential is not part of the cathode or anode, yet we usually know its contribution Ecell-. T F The junction potential represents a balance between unequal ion...
please answer all parts of this question 2. Consider the junction potential a. Describe how and...
please answer all parts of this question
2. Consider the junction potential a. Describe how and why a junction potential occurs. What is the error, in terms of concentration, if a junction potential changes the true b. cell voltage by 1.50 millivolts in a potentiometric determination of an analyte? Show the relevant calculations. c. Describe at least one way in which the error due to a junction potential can be eliminated or at least significantly reduced.
E (Descioe the working prncipie of a vacuum phototube, (ii) Justify whether it can be used in thi...
e (Descioe the working prncipie of a vacuum phototube, (ii) Justify whether it can be used in this instrument. 4. Direct potentiometric analysis requires the use of a pair of electrodes and a voltmeter (a) (i) Write down the reductive half reaction occurs on a silver-silver chloride electrode. (i) Justify whether this electrode can serve as a reference electrode in this method. (b) There is usually a salt bridge at the end of the reference electrode (i) What is the...
Mark Whether are True of False 1. Indicator electrodes are typically made from relatively inert metals...
Mark Whether are True of False 1. Indicator electrodes are typically made from relatively inert metals and they work best when the electrode surface is large and clean 2. Platinum electrodes are more inert than and gold electrodes. 3. KCl is often used as an electrolyte for salt bridge, for the purpose to reduce junction potentials between salt bridges and the electrolyte solutions in cells. 4. Standard conditions for reduction potential’s is 25 °C and = 1 for all aqueous species....
With respect to the membrane potential which of the following is NOT true? A. In resting...
With respect to the membrane potential which of the following is NOT true? A. In resting cells, the membrane potential is negative because sodium ions are less permeable than potassium ions. B. The resting potential of the nerve cell depends on voltage gated potassium channels C. While chloride is much more permeable than sodium, it adds relatively little to the negative membrane potential. D. The concentration of chloride inside/outside the cell is the reciprocal of the potassium concentration of the...
Using the information in the table: Which combination of metals, if used to create an electrochemical...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
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...
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...
Using the table below: 19. Three combinations of metals are listed below, which combination would produce...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
please answer all parts of this question
2. Consider the junction potential a. Describe how and why a junction potential occurs. What is the error, in terms of concentration, if a junction potential changes the true b. cell voltage by 1.50 millivolts in a potentiometric determination of an analyte? Show the relevant calculations. c. Describe at least one way in which the error due to a junction potential can be eliminated or at least significantly reduced.
e (Descioe the working prncipie of a vacuum phototube, (ii) Justify whether it can be used in this instrument. 4. Direct potentiometric analysis requires the use of a pair of electrodes and a voltmeter (a) (i) Write down the reductive half reaction occurs on a silver-silver chloride electrode. (i) Justify whether this electrode can serve as a reference electrode in this method. (b) There is usually a salt bridge at the end of the reference electrode (i) What is the...
Using the information in the table:
Which combination of metals, if used to create an
electrochemical cell, would produce the largest voltage?
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
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...
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...
Using the table below:
19. Three combinations of metals are listed below, which
combination would produce the largest voltage if they were used to
construct an electrochemical cell?
Copper (Cu) with zinc (Zn)
Lead (Pb) with zinc (Zn)
Lead (Pb) with cadmium (Cd)
Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e +...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
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