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
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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...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s)...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
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
KNO, salt bridge Mg Zn Ag 1.0 M Mg 1.0 M Zn2 1.0 M Cu 1.0...
KNO, salt bridge Mg Zn Ag 1.0 M Mg 1.0 M Zn2 1.0 M Cu 1.0 M Ag Reset Info 1.0 M ME LO M 2 1.0 MC 10 MA Reset Set up a cell that has a My electrode in a 1.0 M aqueous Mg? solution on the left side and a Ag electrode in a 1.0 M aqueous A solution on the right side. Add the salt bridge. What is the balanced net ionic equation for this reaction?...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+ (1.0 M) ∣ Zn (s) -0.76 v (iii) Cu2+ (1.0 M) ∣ Cu (s) 0.337 v (iv) Co2+ (1.0 M) ∣ Co (s) -0.28 v Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn - Cu, Zn-Co, and Cu-Co. (the first metal is the anode...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+ (1.0 M) ∣ Zn (s) -0.76 v (iii) Cu2+ (1.0 M) ∣ Cu (s) 0.337 v (iv) Co2+ (1.0 M) ∣ Co (s) -0.28 v Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn - Cu, Zn-Co, and Cu-Co. (the first metal is the anode...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+ (1.0 M) ∣ Zn (s) -0.76 v (iii) Cu2+ (1.0 M) ∣ Cu (s) 0.337 v (iv) Co2+ (1.0 M) ∣ Co (s) -0.28 v Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn - Cu, Zn-Co, and Cu-Co. (the first metal is the anode...
Question 7 (1 point) Standard reduction potentials for the Zn2+/Zn and Pb2+/Pb couples are -0.76 and...
Question 7 (1 point) Standard reduction potentials for the Zn2+/Zn and Pb2+/Pb couples are -0.76 and - 0.13 V, respectively. The galvanic cell below uses the half-cells Pb2+[Pb and Zn2+|Zn, and a salt bridge containing KCl(aq). The voltmeter gives a positive voltage reading. voltmeter salt bridge CD-> The identities of B and D, respectively, are O Pb and Cl- Ozn and Cl- O Pb and K+ O Zn and K+
The following half-cells are availble: (i) Agt (1.0 M) TAg (s) (ii) Zn2+ (1.0 M) |...
The following half-cells are availble: (i) Agt (1.0 M) TAg (s) (ii) Zn2+ (1.0 M) | Zn (s) (iii) Cu2+(1.0 M) Cu(s) (iv) Co2+ (1.0 M) Co (s) 0.7994 v -0.76 v 0.337 v -0.28 v Linking any two half cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn-Cu, Zn-Co, and Cu-Co. (the first metal is the anode and the second is the cathode.)...
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)...
- Zn2+ Choose... Choose... (1pts) Identify the complete redox reaction for a ZnZn2+1|Cu2+1Cu cell. A. Zn(s) + Cu?+ (aq) (aq) + Cu(s) B. Zn(s) + Cu(s) → Zn2+ (aq) + Cu2+ (aq) C. Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) D. Zn (s) + 2 Cu(s) — Zn2+ (aq) + 2 Cu2+ (aq) (1pts) Identify the complete redox reaction for a Zn/Zn2+||Pb2+1Pb cell. A. Zn (s) + Pb(s) Zn2+ (aq) + Pb2+ (aq) B. Zn2+ (aq) + Pb(s) Zn(s)...
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...
KNO, salt bridge Mg Zn Ag 1.0 M Mg 1.0 M Zn2 1.0 M Cu 1.0 M Ag Reset Info 1.0 M ME LO M 2 1.0 MC 10 MA Reset Set up a cell that has a My electrode in a 1.0 M aqueous Mg? solution on the left side and a Ag electrode in a 1.0 M aqueous A solution on the right side. Add the salt bridge. What is the balanced net ionic equation for this reaction?...
Question 7 (1 point) Standard reduction potentials for the Zn2+/Zn and Pb2+/Pb couples are -0.76 and - 0.13 V, respectively. The galvanic cell below uses the half-cells Pb2+[Pb and Zn2+|Zn, and a salt bridge containing KCl(aq). The voltmeter gives a positive voltage reading. voltmeter salt bridge CD-> The identities of B and D, respectively, are O Pb and Cl- Ozn and Cl- O Pb and K+ O Zn and K+
The following half-cells are availble: (i) Agt (1.0 M) TAg (s) (ii) Zn2+ (1.0 M) | Zn (s) (iii) Cu2+(1.0 M) Cu(s) (iv) Co2+ (1.0 M) Co (s) 0.7994 v -0.76 v 0.337 v -0.28 v Linking any two half cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn-Cu, Zn-Co, and Cu-Co. (the first metal is the anode and the second is the cathode.)...
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)...
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