Calculate the standard emf of the following cell at 25 degrees C. Cr(s) ⏐ Cr3+(aq) ⎥⎪ Hg22+(aq) ⏐ Hg(l)
Calculate the standard emf of the following cell at 25 degrees C. Cr(s) ⏐ Cr3+(aq) ⎥⎪...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)
A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate the Gibbs free energy change at 25 °C when 2.61 g of iron is deposited. Assume the concentrations in the cell remain at the standard state values of 1 M through the entire deposition process. Calculate the maximum amount of work done by the cell on its surroundings.
A voltaic cell utilizes the following reaction and operates at 298 K: 3Ce4+(aq)+Cr(s)→3Ce3+(aq)+Cr3+(aq). emf=2.35 1. What is the emf of this cell when [Ce4+]= 1.1 M , [Ce3+]= 1.2×10−2 M , and [Cr3+]=1.1×10−2 M ? 2. when [Ce4+]= 0.40 M ,[Ce3+]= 0.75 M , and [Cr3+]= 1.6 M ?
A voltaic cell utilizes the following reaction and operates at 298 K : 3Ce4+(aq)+Cr(s)→3Ce3+(aq)+Cr3+(aq) Part A What is the emf of this cell under standard conditions? Express your answer using three significant figures. Part B What is the emf of this cell when [Ce4+]= 1.9 M , [Ce3+]= 0.13 M , and [Cr3+]= 1.6×10−2 M ? Express your answer using two significant figures. Part C What is the emf of the cell when [Ce4+]= 7.0×10−3 M ,[Ce3+]= 2.0 M ,...
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
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction and its standard cell potential (in V) at 25°C for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction (please provide)= standard cell potential V= Is the reaction spontaneous at standard conditions?
Consider a galvanic electrochemical cell constructed using Cr/Cr3* and Zn/Zn2+ at 25 °C. The following half-reactions are provided for each metal: Cr3+ (aq) + 3 e → Cr(s) Eºred = -0.744 V Zna*(aq) + 2 e Zn(s) Eºred = -0.763 V What is the standard cell potential for this cell?
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions?_____ V (b) What is the emf of this cell when [Ce4+] = 1.3 M, [Ce3+] = 0.013 M, and [Cr3+] = 0.014 M?_____ V (c) What is the emf of the cell when [Ce4+] = 0.51 M, [Ce3+] = 0.88 M, and [Cr3+] = 1.2 M? _____V
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? _V (b) What is the emf of this cell when [Ce4+] = 1.8 M, [Ce3+] = 0.013 M, and [Cr3+] = 0.015 M? _V (c) What is the emf of the cell when [Ce4+] = 0.56 M, [Ce3+] = 0.85 M, and [Cr3+] = 1.4 M? _V
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? _____V (b) What is the emf of this cell when [Ce4+] = 1.2 M, [Ce3+] = 0.010 M, and [Cr3+] = 0.012 M? ____V (c) What is the emf of the cell when [Ce4+] = 0.53 M, [Ce3+] = 0.89 M, and [Cr3+] = 1.0 M? ____V