When doing a Nernst equation, how do you calculate n? I know for something like Zn|Zn2+(1.0...
When doing a Nernst equation, how do you calculate n? I know for something like
|
Zn|Zn2+(1.0 M)||Cu2+(1.0 M)|Cu |
|---|
where you have 2+ and 2+ n would be 2, but what about something like
|
Pb|Pb2+(1.0 M)||Ag+(0.10 M)|Ag |
|---|
where you have 2+ and +
I'm confused and can't find an answer anywhere
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When doing a Nernst equation, how do you calculate n? I know for
something like
Zn|Zn2+(1.0...
Need to find the Reaction Quotient for the following: 7.Zn|Zn2+(1.0 M)||Ag+(0.10 M)|Ag 8.Zn|Zn2+(0.10 M)||Ag+(0.10 M)|Ag 12.Pb|Pb2+(1.0...
Need to find the Reaction Quotient for the following: 7.Zn|Zn2+(1.0 M)||Ag+(0.10 M)|Ag 8.Zn|Zn2+(0.10 M)||Ag+(0.10 M)|Ag 12.Pb|Pb2+(1.0 M)||Ag+(0.10 M)|Ag 14.Cu|Cu2+(1.0 M)||Ag+(0.10 M)|Ag
Use the table of Standdard Reduction Potentials and the Nernst Equation to calculate the concentration of...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
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...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
how do i do nerst equation 1. Standard Cells Voltaie Cell Data Sheet Experimental Cell Potential,...
how do i do nerst equation
1. Standard Cells Voltaie Cell Data Sheet Experimental Cell Potential, volts Calculated Cell Potential volts =.47 v PbPb (1.0 MIC"(1.0 MC SnSn" (1.0 M) "(1.0 M) = 485 ,465 540 .44v 08v CujCư"(1.0 M)||Ag (1,0 M)/AS - ,460 Sn/Sn?"(1.0 M)||Pb (1.0M)/Pb Olv Pb/Pb2+(1.0 M)||Ag" (1.0 MAS 93 Sn/Sn? (1.0 M)||Ag (1.0 M)/Ag 19/ -99 = 94v 80 II. Nonstandard Cells Voltaic Cell Experimental Cell Potential, volts Calculated Potential, Nernst Equation, volts* Pb/Pb*P(1.0 M)||Cu?(0.0010 M)|Cu...
Class Practice C152-02 Chapter 21 Practice 4 Calculate the reduction potential of the Cu2/Cu electrode when...
Class Practice C152-02 Chapter 21 Practice 4 Calculate the reduction potential of the Cu2/Cu electrode when [Cu] - 1.0 x108 M. (hint: use the table of standard reduction potentials and the Nernst Equation) A cell is constructed by immersing a strip of silver in 0.10 M AgNO, solution and a strip of lead in 1.0 M Pb(NO) solution. A wire and salt bridge complete the cell. What is the potential for the cell? (hint: use the Nernst Equation to determine...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq,...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value...
Use the Nernst equation to calculate the theoretical value of E of th copper-concentration cell and compare this value with th cell potential you measured. E = E* - 0.0592 / n * logQ **So I believe this is the equation that I would use. However, i'm don't know what E* is suppose to be...** The my electrochemistry experiment the cell potential that i measured were: 0.130V, 0.115V, and 0.110V (average cell potential = 0.118V) The concentration of the copper...
The following two reactions have ξ values given below 4°-2.07 V If the potential for the reaction...
*Electrochemistry
Plase check my answers! Are these right??
Help me!
The following two reactions have ξ values given below 4°-2.07 V If the potential for the reaction pt2t following half reactions. 2e Pt is assigned a value of zero, calculate the cell potentials for the a. Ag+e-Ag -0.40V 0,4 ov 0+0.40 # b. F2cF 5.oV 4. Consider the galvanic cell at 25°C Zn Zn2 I Cu2+ Cu Calculate the ratio of IZn2+1 to [Cu2+1 when the cell potential has dropped...
1. How do I read the half reaction table? 2. If im asked for the best...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
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...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
how do i do nerst equation
1. Standard Cells Voltaie Cell Data Sheet Experimental Cell Potential, volts Calculated Cell Potential volts =.47 v PbPb (1.0 MIC"(1.0 MC SnSn" (1.0 M) "(1.0 M) = 485 ,465 540 .44v 08v CujCư"(1.0 M)||Ag (1,0 M)/AS - ,460 Sn/Sn?"(1.0 M)||Pb (1.0M)/Pb Olv Pb/Pb2+(1.0 M)||Ag" (1.0 MAS 93 Sn/Sn? (1.0 M)||Ag (1.0 M)/Ag 19/ -99 = 94v 80 II. Nonstandard Cells Voltaic Cell Experimental Cell Potential, volts Calculated Potential, Nernst Equation, volts* Pb/Pb*P(1.0 M)||Cu?(0.0010 M)|Cu...
Class Practice C152-02 Chapter 21 Practice 4 Calculate the reduction potential of the Cu2/Cu electrode when [Cu] - 1.0 x108 M. (hint: use the table of standard reduction potentials and the Nernst Equation) A cell is constructed by immersing a strip of silver in 0.10 M AgNO, solution and a strip of lead in 1.0 M Pb(NO) solution. A wire and salt bridge complete the cell. What is the potential for the cell? (hint: use the Nernst Equation to determine...
Candidate l: Zn(s) | Zn2+(aq,0.500 M) I Cu2+(aq, 1.00 M) Cu(s) Candidate 2: Pb(s) | Pb2+(aq, 0.500 M) || Cu2+(aq, 1.00 M) Cu(s) Candidate 3: Mg(s) | Mg2+(aq, 0.500 M) | Pb2+(aq, 1.00 M)| Pb(s) (a) 6 pts) Choose one of the candidate voltaic cells #1, #2, or #3. Draw a schematic cell diagram for the candidate voltaic cell of choice. Clearly label anode, cathode, electrodes, ions and their concentrations, salt bridge, and the flow of electrons. (b) (5 pts)...
*Electrochemistry
Plase check my answers! Are these right??
Help me!
The following two reactions have ξ values given below 4°-2.07 V If the potential for the reaction pt2t following half reactions. 2e Pt is assigned a value of zero, calculate the cell potentials for the a. Ag+e-Ag -0.40V 0,4 ov 0+0.40 # b. F2cF 5.oV 4. Consider the galvanic cell at 25°C Zn Zn2 I Cu2+ Cu Calculate the ratio of IZn2+1 to [Cu2+1 when the cell potential has dropped...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
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