Consider the following balanced cell reaction: &nb
Consider the following balanced cell reaction:
Cr2O72- + 14H+ + 6I- ⟶ 2Cr3+ + 3I2+ 7H2O
In the determination of the cell potential at nonstandard conditions, the value that should be used for “n” (i.e. number of electrons transferred) in the Nernst equation is:
A. 2
B. 6
C. 1
D. 4
E. 5
Homework Answers
Consider the following balanced cell reaction: Cr20,2 + 14H+ +61 -2Cr3+ + 312 + 7H,0 In...
Consider the following balanced cell reaction: Cr20,2 + 14H+ +61 -2Cr3+ + 312 + 7H,0 In the determination of the cell potential at nonstandard conditions, the value that should be used for "n" (i.e. number of electrons transferred) in the Nernst equation is: O 2 1 5
Calculate the standard cell potential for each of the following electrochemical cells. You may want to...
Calculate the standard cell potential for each of the following electrochemical cells. You may want to reference (Pages 854 - 861) Section 19.4 while completing this problem. a) Cr2O72−(aq)+14H+(aq)+6I−(aq)→2Cr3+(aq)+7H2O(l)+3I2(s)
Could someone please explain how to do this question? Thanks! Select the balanced equation for the...
Could someone please explain how to do this question?
Thanks!
Select the balanced equation for the reaction of K2Cr2O7 and FeSO4 in an acidic aqueous solution: o a. 2 Select one: a. Cr20-2- +6Fe2+ = 2Cr3+ + 6Fe3+ b. 14H+ + Cr2O72- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ c. 7H2+ + Cr20-2- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ d. 14H+ + 2Cr20-2- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ O e. 7H+ + Cr2O72- +...
Choose the label which best describes the following: A B C D E F G H Direction...
Choose the label which best describes the following:
A B C D E F G H Direction which anions move through the
salt bridge
A B C D E F G H Pt anode
The overall, balanced, spontaneous reaction occurring in this
(standard) cell is:
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq) → 7H2O(l) + 2Cr3+(aq) +
3Cl2(g)
7H2O(l) + 2Cr3+(aq) + 3Cl2(g) →
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq)
7H2O(l) + 2Cr3+(aq) + Cl2(g) →
Cr2O72−(aq) + 2Cl−(aq)
+ 14H+(aq)
2Cr3+(aq) + 3Cl2(g) →...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e →...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e → Zn -0.76 Au?+ + 3e → Au 1.50 If this cell is set up at 25°C with [Zn2] = 1.00 x 10-4M and [Au?') -2.00 10-2M, the expected cell potential is Submit Hide Hints Hint 1 Hint 2 The Nernst equation is based on the balanced cell reaction. Q reflects the mass action expression for the balanced cell reaction and n is the number...
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....
A voltaic cell uses the following reaction: 2Al(s) + 3I2(s) → 2Al3+(aq) + 6I-(aq) a) Calculate...
A voltaic cell uses the following reaction: 2Al(s) + 3I2(s) → 2Al3+(aq) + 6I-(aq) a) Calculate the cell potential (ε°cell) under standard conditions. b) Calculate the cell potential (E) when [Al3+] = 0.015M and [I-] = 0.025M.
pleas help me with lab assament Multimeter Consider a galvanic cell consisting of the following two...
pleas help me with lab assament
Multimeter Consider a galvanic cell consisting of the following two redox couples: Ag+(0.010 M) + e-→ Ag(s) Eo = +0.80 V oi a. Write the equation for the half-reaction occurring at the Salt bridge C (0.010 M) Ag (0.010AM b. Write the equation for the half-reaction occurring at the anode. Cr Ag c. Write the equation for the cell reaction. d. What is the standard cell potential, Eelli for the cell? e. Realizing the...
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu...
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...
all parts please cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+...
all parts please
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: (Ag +) = 2.0 M; [Cu 2+] = 0.025 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is...
Consider the following balanced cell reaction: Cr20,2 + 14H+ +61 -2Cr3+ + 312 + 7H,0 In the determination of the cell potential at nonstandard conditions, the value that should be used for "n" (i.e. number of electrons transferred) in the Nernst equation is: O 2 1 5
Could someone please explain how to do this question?
Thanks!
Select the balanced equation for the reaction of K2Cr2O7 and FeSO4 in an acidic aqueous solution: o a. 2 Select one: a. Cr20-2- +6Fe2+ = 2Cr3+ + 6Fe3+ b. 14H+ + Cr2O72- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ c. 7H2+ + Cr20-2- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ d. 14H+ + 2Cr20-2- + 6Fe2+ → 2Cr3+ + 7H2O + 6Fe3+ O e. 7H+ + Cr2O72- +...
Choose the label which best describes the following:
A B C D E F G H Direction which anions move through the
salt bridge
A B C D E F G H Pt anode
The overall, balanced, spontaneous reaction occurring in this
(standard) cell is:
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq) → 7H2O(l) + 2Cr3+(aq) +
3Cl2(g)
7H2O(l) + 2Cr3+(aq) + 3Cl2(g) →
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq)
7H2O(l) + 2Cr3+(aq) + Cl2(g) →
Cr2O72−(aq) + 2Cl−(aq)
+ 14H+(aq)
2Cr3+(aq) + 3Cl2(g) →...
Consider a galvanic cell based on the following half reactions: E° (V) Zn2+ + 2e → Zn -0.76 Au?+ + 3e → Au 1.50 If this cell is set up at 25°C with [Zn2] = 1.00 x 10-4M and [Au?') -2.00 10-2M, the expected cell potential is Submit Hide Hints Hint 1 Hint 2 The Nernst equation is based on the balanced cell reaction. Q reflects the mass action expression for the balanced cell reaction and n is the number...
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....
pleas help me with lab assament
Multimeter Consider a galvanic cell consisting of the following two redox couples: Ag+(0.010 M) + e-→ Ag(s) Eo = +0.80 V oi a. Write the equation for the half-reaction occurring at the Salt bridge C (0.010 M) Ag (0.010AM b. Write the equation for the half-reaction occurring at the anode. Cr Ag c. Write the equation for the cell reaction. d. What is the standard cell potential, Eelli for the cell? e. Realizing the...
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...
all parts please
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: (Ag +) = 2.0 M; [Cu 2+] = 0.025 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is...
Most questions answered within 3 hours.
-
Write the net ionic equation for the precipitation reaction that
occurs when aqueous solutions of aluminum...
asked 39 seconds ago -
How do we find the slope distance, given the horizontal distance
and the zenith angle?
For...
asked 46 seconds from now -
The table to the right lists probabilities for the corresponding
numbers of girls in three births....
asked 10 minutes ago -
The inverse demand function for good X is P = 5−0.05Q. The
firm’s cost curve is...
asked 9 minutes ago -
The Fresh Connection is really pushing the new line of juice
products. Given that it takes...
asked 14 minutes ago -
An acute decrease in mean arterial pressure (by getting up very
quickly, for instance) will cause...
asked 13 minutes ago -
Is the pH of solutions important when using the Fluoride ISE? If
so, why?
asked 17 minutes ago -
Producer surplus is:
a.
always equal to consumer surplus.
b.
the amount paid to sellers above...
asked 18 minutes ago -
In 2005, Derrek Lee led the National Baseball League with a
0.335 batting average, meaning that...
asked 37 minutes ago -
Write a recursive function moreFactors(a,b,fact) that does the
following:
1. Takes as an input 3 positive...
asked 36 minutes ago -
In order for corporations to behave ethically, they must,
ultimately, give up the profit motive.
...
asked 37 minutes ago -
Blue Spruce Corp. owns equipment that cost $63,400 when
purchased on January 1, 2017. It has...
asked 57 minutes ago