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For a voltaic cell based on the reaction below, what reaction happens at the anode? 2Ni3+(aq)+Cd(s)→2Ni2+(s)+Cd2+(aq)...
For a voltaic cell based on the reaction below, what reaction happens at the anode? 2Ni3+(aq)+Cd(s)→2Ni2+(s)+Cd2+(aq) Ni3+(aq)+e-→Ni2+(aq) Ni2+(aq)→ Ni3+(aq)+e- Cd2+(aq)+2e-→Cd(s) Cd(s)→Cd2+(aq)+2e- A student measures the voltage across different metal electrodes placed in a voltaic cell. Using a copper cathode, the voltages when using a first a tin, then gold anode are positive and negative, respectively. The order of chemical reactivity of the solid metals must be Au>Cu>Sn Au=Sn Sn>Cu>Au Au=Sn>Cu
Enter electrons as e A voltaic cell is constructed in which the anode is a Mg...
Enter electrons as e A voltaic cell is constructed in which the anode is a Mg Mg2+ half cell and the cathode is a Ni Ni2+ half cell. The half- cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + €...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + V> + The net cell reaction is:...
19 20 Question 16 Half-cell Potentials: Half Reaction: E' value + 0.80 V +0.77 V Agte...
19 20 Question 16 Half-cell Potentials: Half Reaction: E' value + 0.80 V +0.77 V Agte → AS Fe3+ + + Fe2+ Cu2+ 2e → Cu Pb2+ + 2e → Pb +0.34 V -0.13 V Ni2+ + 2e → NI -0.25 V - 0.40 V Cd2+ +2e → ca Fe2+ + 2e → Fe Zn2+ + 2e → Zn -0.44 V - 0.76 V A13+ +3 → AI - 1.66 V Consider an electrochemical cell constructed from the following half...
Given the following information: Ni2+ + 2e- Ni(s) Eº = -0.25 V Ag* + e. Ag(s)...
Given the following information: Ni2+ + 2e- Ni(s) Eº = -0.25 V Ag* + e. Ag(s) E° = 0.80 V 1) Determine the cell potential of the spontaneous redox reaction. 2) Give the net ionic equation for the overall balanced redox reaction. 3) Label the Galvanic Cell below to model the reaction above. Please include: • substances in each compartment • the salt bridge • the anode • the cathode 4) Give the line notation representation of this galvanic cell....
A) B) C) Enter electrons as e. Use smallest possible integer coefficients for ALL reactions. If...
A)
B)
C)
Enter electrons as e. Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Cl2(g) + Hg(1) —→ 2CH(aq) + Hg2+(aq) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate the C-Cl, electrode | y the Hg|Hg2+ electrode. In the salt bridge, anions migrate...
2. Answer each of the following: (i) Explain using VSEPRT the difference in geometries of CH4...
2. Answer each of the following: (i) Explain using VSEPRT the difference in geometries of CH4 and H20. [4 Marks] (ii) Discuss the energy of the valence and conductance bands in conductors, insulators and semiconductors. Outline the chemical basis for p and n-doped semiconductors [10 Marks] (iii) Nickel-cadmium (Ni-cad) batteries are rechargeable and are commonly used in cordless appliances. Although such batteries actually function under basic conditions, imagine an electrochemical cell using the setup below. V Cd Ni Salt Bridge...
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110...
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110 The half cell and the reuction potential for the anode is: Half-Reaction E (V) Ni2+ (aq) + 2e ® Ni(s) -0.25 Using this information from the diagram, determine the standard reduction potential of metal M. +0.25 V O-1.40V +0.80 v -0.80 V +1.40 V
Part A Describe a galvanic cell that uses the reaction: 2Ag+ (aq) + Ni(s) + 2Ag(s)...
Part A Describe a galvanic cell that uses the reaction: 2Ag+ (aq) + Ni(s) + 2Ag(s) + Ni2+ (aq) Match the items in the left column to the appropriate blanks in the sentences on the right Reset Help Nja: Ag There is an anode in an aqueous solution of and an cathode in an aqueous solution of A connects the anode and cathode compartment. The electrodes are connected through an external circuit Ag semiconductor Ni salt bridge dielectric Write the...
Enter electrons as e A voltaic cell is constructed in which the anode is a Mg Mg2+ half cell and the cathode is a Ni Ni2+ half cell. The half- cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + V> + The net cell reaction is:...
19 20 Question 16 Half-cell Potentials: Half Reaction: E' value + 0.80 V +0.77 V Agte → AS Fe3+ + + Fe2+ Cu2+ 2e → Cu Pb2+ + 2e → Pb +0.34 V -0.13 V Ni2+ + 2e → NI -0.25 V - 0.40 V Cd2+ +2e → ca Fe2+ + 2e → Fe Zn2+ + 2e → Zn -0.44 V - 0.76 V A13+ +3 → AI - 1.66 V Consider an electrochemical cell constructed from the following half...
Given the following information: Ni2+ + 2e- Ni(s) Eº = -0.25 V Ag* + e. Ag(s) E° = 0.80 V 1) Determine the cell potential of the spontaneous redox reaction. 2) Give the net ionic equation for the overall balanced redox reaction. 3) Label the Galvanic Cell below to model the reaction above. Please include: • substances in each compartment • the salt bridge • the anode • the cathode 4) Give the line notation representation of this galvanic cell....
A)
B)
C)
Enter electrons as e. Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Cl2(g) + Hg(1) —→ 2CH(aq) + Hg2+(aq) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate the C-Cl, electrode | y the Hg|Hg2+ electrode. In the salt bridge, anions migrate...
2. Answer each of the following: (i) Explain using VSEPRT the difference in geometries of CH4 and H20. [4 Marks] (ii) Discuss the energy of the valence and conductance bands in conductors, insulators and semiconductors. Outline the chemical basis for p and n-doped semiconductors [10 Marks] (iii) Nickel-cadmium (Ni-cad) batteries are rechargeable and are commonly used in cordless appliances. Although such batteries actually function under basic conditions, imagine an electrochemical cell using the setup below. V Cd Ni Salt Bridge...
Consider the following electrochemical cell at room temperature. 1.05 V N м Salt Bridge Ni2+an (110 The half cell and the reuction potential for the anode is: Half-Reaction E (V) Ni2+ (aq) + 2e ® Ni(s) -0.25 Using this information from the diagram, determine the standard reduction potential of metal M. +0.25 V O-1.40V +0.80 v -0.80 V +1.40 V
Part A Describe a galvanic cell that uses the reaction: 2Ag+ (aq) + Ni(s) + 2Ag(s) + Ni2+ (aq) Match the items in the left column to the appropriate blanks in the sentences on the right Reset Help Nja: Ag There is an anode in an aqueous solution of and an cathode in an aqueous solution of A connects the anode and cathode compartment. The electrodes are connected through an external circuit Ag semiconductor Ni salt bridge dielectric Write the...
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