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Given the following data: PtCL2 (aq) + 2ePt(s)+ 4CI'(aq) Pt2 (aq)+ 4CI(aq) PtCl (aq) E° +0.73...
You intend to construct a very expensive) battery using PtCl2/Pt and AgNO3/Ag as your materiais Which...
You intend to construct a very expensive) battery using PtCl2/Pt and AgNO3/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl(aq) + 2e - Pt(s) + 2 Cl. (aq) E' = +1.20 V AgNO3 (aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl (aq) + 2e - Pt(s) + 2 Cl. (aq) E= +1.20 V AgNO3(aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall reaction...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered = -0.23 V Pt2+ (aq) + 2e-E Pt(s), Ered = +1.2 V Pd2+(aq) + 2e- EPd(s), Ered = 0.99 V a) Sketch the cell for which the overall cell potential is the greatest. [3 Marks) b) Identify the cathode and anode, and then show the direction of electron flow for the cell in the circuit (a). [3 Marks] c) Will Pt(s) reduce Pd2+(aq)? Explain...
Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following...
Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following Eo values: Ca2+(aq)+2e−→Ca(s) Eo = -2.02 V Mn2+(aq)+2e−→Mn(s) Eo = -1.41 V
Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following...
Calculate the cell potential, the equilibrium constant, and the free-energy change for: Ca(s)+Mn2+(aq)(1M)⇌Ca2+(aq)(1M)+Mn(s) given the following Eo values: Ca2+(aq)+2e−→Ca(s) Eo = -1.59 V Mn2+(aq)+2e−→Mn(s) Eo = -0.54 V 1.) Calculate the equilibrium constant. 2.) Free-energy change?
Given that Eºcell is 0.62 V for the following cell TI(s) | T|3+ (aq) || CI(aq)...
Given that Eºcell is 0.62 V for the following cell TI(s) | T|3+ (aq) || CI(aq) | Cl2(g) | Pt(s) and that the standard reduction potential for the half-reaction Cl2(g) + 2e - →2C1-(aq) is 1.36 V, calculate the standard reduction potential for the half-reaction T13+(aq) + 3e → Tl(s). 0.74 V -1.98 V -0.74 V +1.98 V +0.12 V
Given the two following half reactions, Cr(aq) + 3e- → Cr(s) E° = -0.74 V Hg2(aq)...
Given the two following half reactions, Cr(aq)
+ 3e- → Cr(s) E° = -0.74 V Hg2(aq)
+ 2e- → Hg(l) E° = +0.80 V calculate the standard emf for the
following cell: Cr | Cr||
Hg2|
Hg
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V...
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V Cult(aq) + e + Cu(s) E° = 0.521 v Determine the half-cell reactions and the overall cell reaction, calculate the cell potential, and determine the equilibrium constant at 298.5 K for the cell: Pt (8)| H2(g)| H+(aq, ah+ = 0.25)||Cu²+( aq, acu2+ = 0.10) Cu(s) Is the cell reaction spontaneous as written?
What is the equilibrium constant for the following reaction at 298 K? 2 Ag+(aq) + 2...
What is the equilibrium constant for the following reaction at 298 K? 2 Ag+(aq) + 2 I-(aq) → I2(s) + 2 Ag(s) Eº = +0.265 V Group of answer choices 2.99 x 104 1.60 x 107 9.04 x 108 87.9 7.73 x 103 Using data from the reduction potential table below and the reaction 2 Ag(s) + Pt2+(aq) → Pt(s) + 2 Ag+(aq) Eº = 0.38 V calculate the standard reduction potential of the half-reaction Pt2+(aq) + 2 e- →...
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s)...
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s) Eo= 0.8V If you increase the concentration of Cu2+(aq), which of the following would be true about the cell potential E? It would remain constant It would increase It would decrease This cannot be determined
You intend to construct a very expensive) battery using PtCl2/Pt and AgNO3/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl(aq) + 2e - Pt(s) + 2 Cl. (aq) E' = +1.20 V AgNO3 (aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall...
You intend to construct a very expensive battery using PtCl2/Pt and AgNO/Ag as your materiais Which half-reaction is the anode, and which is the cathode? PtCl (aq) + 2e - Pt(s) + 2 Cl. (aq) E= +1.20 V AgNO3(aq) + e - Ag (s) + NO3- (aq) E = +0.80 V Explain how you determined the appropriate half reaction for the anode. Calculate Ecall for the battery you have constructed. Ecell = Write the balanced equation for the overall reaction...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered = -0.23 V Pt2+ (aq) + 2e-E Pt(s), Ered = +1.2 V Pd2+(aq) + 2e- EPd(s), Ered = 0.99 V a) Sketch the cell for which the overall cell potential is the greatest. [3 Marks) b) Identify the cathode and anode, and then show the direction of electron flow for the cell in the circuit (a). [3 Marks] c) Will Pt(s) reduce Pd2+(aq)? Explain...
Given that Eºcell is 0.62 V for the following cell TI(s) | T|3+ (aq) || CI(aq) | Cl2(g) | Pt(s) and that the standard reduction potential for the half-reaction Cl2(g) + 2e - →2C1-(aq) is 1.36 V, calculate the standard reduction potential for the half-reaction T13+(aq) + 3e → Tl(s). 0.74 V -1.98 V -0.74 V +1.98 V +0.12 V
Given the two following half reactions, Cr(aq)
+ 3e- → Cr(s) E° = -0.74 V Hg2(aq)
+ 2e- → Hg(l) E° = +0.80 V calculate the standard emf for the
following cell: Cr | Cr||
Hg2|
Hg
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V Cult(aq) + e + Cu(s) E° = 0.521 v Determine the half-cell reactions and the overall cell reaction, calculate the cell potential, and determine the equilibrium constant at 298.5 K for the cell: Pt (8)| H2(g)| H+(aq, ah+ = 0.25)||Cu²+( aq, acu2+ = 0.10) Cu(s) Is the cell reaction spontaneous as written?
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