Concept explainers
Interpretation:
The emf of theconcentration cell at
Concept introduction:
The solubility product,
Here,
The standard reduction potential of a galvanic cell may be calculated in terms of the standard reduction potential of cathode and anode as the relation mentioned below.
Here,
Reaction quotient is the ratio of the molar concentration of the ions in the products to that of the reactants, raised to the power of their stoichiometric coefficients.
According to the Nernst equation, the relation between emf, standard cell potential, and reaction quotient, at
Here,
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- When the Pb2+ concentration is 1.28 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.362V. What is the Mg2+ concentration?Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq)Answer: _________ Marrow_forwardWhen the Ag+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.658V. What is the Zn2+ concentration? 2Ag+(aq) + Zn(s)2Ag(s) + Zn2+(aq) Answer: M Submit Answerarrow_forwardWhat is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 7.14×10-4 M and the Mg2+ concentration is 1.35 M? Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:arrow_forward
- What is the equilibrium constant, K, at 298 K for the spontaneous cell made from the following half-cell reactions? Cr3+(aq) + 3e– → Cr(s) E° = –0.73 V Ag+(aq) + e– → Ag(s) E° = 0.80 V Express your answer to two significant figures. K = Answerarrow_forwardCalculate the cell potential of a voltaic cell given the following standard potentials: X -> X2+ + 2 e- Eo = -1.69 V Y3+ -> + 3 e- -> Y Eo = 0.94 V Note: Answer in 2 decimal places.arrow_forward(a) How many coulombs are required to plate a layer of nickel metal 0.125 mm thick on a coin with a diameter of 3 cm from a solution containing nickel ions? The density and atomic weight of nickel metal is 8.908 g/cm3 and 58.693 g /mol, respectively. Answer (b) What current flow in amperes is required for this electroplating if the coin is to be plated in 5 mins. ? Answer (c) If the external source has an emf of +9.0 V and the electrolytic cell is 75% efficient, how much electrical power in W is expended to electroplate the coin? Answer HINT: Use 96480 C = 1 mol e- and express your final answer in 3 decimal places.arrow_forward
- Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25∘C and standard conditions of 1 MM for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E∘−(2.303RT/nF) log10Q where E is the potential in volts, E∘ is the standard potential at 25 ∘C in volts, R=8.314J/(K⋅mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e−) is the Faraday constant, and Q is the reaction quotient. At the common reference temperture of 298 K, substituting each constant into the equation the result is E=E∘−(0.0592 V/n)log10Q a) Calculate the standard cell potential at 25 ∘C for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) b) What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 57 ∘C when [Fe2+]= 3.80 MM and [Mg2+]= 0.210 MM .arrow_forwardWhen the Ag+ concentration is 5.25×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.975V. What is the Mg2+ concentration?2Ag+(aq) + Mg(s)--->2Ag(s) + Mg2+(aq)Answer: _____Marrow_forwardExercise Electrochemistry For the following cell at 298 K: Cu (s) I Cu2 + (aq) II Ag + (aq) I Ag (s) a) Write the reaction that occurs, given that the element with the largest standard reduction potential is reduced. b) Write the Nernst reaction for the cell. c) Calculate the potential when the ions present have activity 0.1.arrow_forward
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