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You are given a solution and are informed that the concentration of the species is [Fe...
can you please help.me answer these three questions please? I am really desperate and in need...
can you please help.me answer these three questions
please? I am really desperate and in need of help.
Question 10 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and Al3+ (aq)/Al(s) electrodes. Ni2+(aq) + 2e - Ni(s) Ered = -0.257 V Al3+(aq) + 3e Al(s) Eºred = -1.676 V Calculate AG° 0 -273.9 kJ ho O-821.6 kJ 0 -410.8 kJ +821.6 kJ O +273.9 kJ Question 11 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and...
What is the standard cell potential of a cell created using a cadmium electrode in 0.45...
What is the standard cell potential of a cell created using a cadmium electrode in 0.45 M Cd(NO3)2(aq) and a graphite electrode in an aqueous solution that is 0.45 M in both Fe2+ and Fe3+? 0.38 V 1.95 V 1.94 V 1.17 V 1.18 V What is the standard cell potential of a cell which utilizes the following reaction: Zn (s) + Ni2+ (aq) → Ni (s) + Zn2+ (aq) All solutions are 1.0 M and the reaction occurs at...
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Expre...
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Express your answer to three significant figures and in units of kJ/mol. Consider constructing a voltaic cell with one compartment containing a Zn(s) electrode immersed in a Zn2+ aqueous solution and the other compartment containing an Al(s) electrode immersed in an Al3+ aqueous solution. What is the spontaneous reaction in this cell? Group of answer choices Zn + Al3+ → Al...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.80 molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V A) What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? B) What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.60molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V Part A What is the initial cell potential? Part B What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? Part C What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
For the electrochemical cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode?...
For the electrochemical cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s) Zn(s) → Zn2+(aq) + 2 e- o Zn2+(aq) + 2 e- → Zn(s) + Ni(s) → Ni2+(aq) + 2 e- Ni2+(aq) + 2 e- → Ni(s)
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 =...
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 +...
37. What is the Ecell at 25°C for the following reaction and is it spontaneous? Zn(s)...
37. What is the Ecell at 25°C for the following reaction and is it spontaneous? Zn(s) + Ni2+ (aq, 10-4 mol L ) → Zn2+ (aq, 0.1 mol L"!) + Ni(s) Ni2+ (aq) + 2e → Ni(s) E"=-0.44 V Zn²+(aq) + 2e → Zn(s) E'= -0.76 V b) 0.32 V, Spontaneous 0.41 V, Spontaneous -0.32 V, Not spontaneous -0.23 V, Not spontaneous 0.23 V, Spontaneous e)
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] =...
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.839 M and [Ni2+] = 0.0150 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+(aq) = Zn2+ (aq) + Ni(s) E = V
can you please help.me answer these three questions
please? I am really desperate and in need of help.
Question 10 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and Al3+ (aq)/Al(s) electrodes. Ni2+(aq) + 2e - Ni(s) Ered = -0.257 V Al3+(aq) + 3e Al(s) Eºred = -1.676 V Calculate AG° 0 -273.9 kJ ho O-821.6 kJ 0 -410.8 kJ +821.6 kJ O +273.9 kJ Question 11 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and...
What is the standard cell potential of a cell created using a cadmium electrode in 0.45 M Cd(NO3)2(aq) and a graphite electrode in an aqueous solution that is 0.45 M in both Fe2+ and Fe3+? 0.38 V 1.95 V 1.94 V 1.17 V 1.18 V What is the standard cell potential of a cell which utilizes the following reaction: Zn (s) + Ni2+ (aq) → Ni (s) + Zn2+ (aq) All solutions are 1.0 M and the reaction occurs at...
For the electrochemical cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s) Zn(s) → Zn2+(aq) + 2 e- o Zn2+(aq) + 2 e- → Zn(s) + Ni(s) → Ni2+(aq) + 2 e- Ni2+(aq) + 2 e- → Ni(s)
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 =...
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 +...
37. What is the Ecell at 25°C for the following reaction and is it spontaneous? Zn(s) + Ni2+ (aq, 10-4 mol L ) → Zn2+ (aq, 0.1 mol L"!) + Ni(s) Ni2+ (aq) + 2e → Ni(s) E"=-0.44 V Zn²+(aq) + 2e → Zn(s) E'= -0.76 V b) 0.32 V, Spontaneous 0.41 V, Spontaneous -0.32 V, Not spontaneous -0.23 V, Not spontaneous 0.23 V, Spontaneous e)
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.839 M and [Ni2+] = 0.0150 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+(aq) = Zn2+ (aq) + Ni(s) E = V
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