Electrochemical Measurement of Concentration
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode.
What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 9.2×10-5 M?
1 pts
Tries 0/8 |
The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.160 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.)
1 pts
Tries 0/8 |
A calibration curve to show how the cell potential varies with [Cu2+] may be constructed. A plot of cell potential (in V, with the same sense as in question 1) versus log10[Cu2+] should yield a straight line. What is the slope of this line?
Electrochemical Measurement of Concentration
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode.
What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 9.2×10-5 M?
1 pts
Tries 0/8 |
The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.160 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.)
1 pts
Tries 0/8 |
A calibration curve to show how the cell potential varies with [Cu2+] may be constructed. A plot of cell potential (in V, with the same sense as in question 1) versus log10[Cu2+] should yield a straight line. What is the slope of this line?
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a) What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 7.5×10-8 M? b) The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.109 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.) c) A calibration curve...
Please show all work step by step and final answer. Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 3.6x10-4 M? 1 pts Submit Answer Tries 0/5 The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.136...
Please show all work step by step and final answer. Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 3.2x10-6 M? 1 pts Submit Answer Tries 0/5 The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.038...
Please answer ALL THREE PARTS of the question with correct answers and explanations. Thanks. Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 1.9x10-9 M? 1pts Submit Answer Tries 0/5 The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at...
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which = 3.8 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown (Cu?+]. The measured potential at 25°C is 0.206 v. What is (cu?+]? (Assume Cu²+ is reduced.) [Cu²+] = M
Please answer only if you know it. Thanks. An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which 9.0 x 10-5 M? Ecell = v b. The copper electrode is placed in a solution of unknown The measured potential at 25°C is 0.177 V. What is ? (Assume Cu2+ is reduced.)
question iii 10. An electrochemical cell consists of a standard Fe/Fe electrode (Fe (aq) (1.OM) IFe (aq) (1.0M) IPt(s) and a copper metal electrode ( concentrations) Cu2 (aq) +2e Cu(s) Fe (aq) le Fe (aq) +0.34 V -034 +0.77V Mark what is the corect balanced equation for the spontaneous reac u (aq) Fe (aq) Cu(s)+Fe2 (aq) C) Cu(s) + Fe (aq) Cu (aq) + Fe (aq) α Cu2+(aq) + 2e → Cu(s) + Fe2+(aq) Cu → Cu2ト+20 94 i) (...
In this lab you will construct several electrochemical cells where both half-cells contain a copper electrode in a copper (II) solution. What standard cell potential (Eocell) would be expected for a voltaic cell comprised only of copper? Question 7 1 pts In this lab you will construct several electrochemical cells where both half-cells contain a copper electrode in a copper (II) solution. What standard cell potential (Eºcell would be expected for a voltaic cell comprised only of copper? O 0.68...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
An electrochemical cell is constructed such that on one side a pure nickel electrode is in contact with a solution containing Ni2+ ions at a concentration of 5*10-3 M. The other cell half consists of a pure Fe electrode that is immersed in a solution of Fe2+ ions having a concentration of 0.3 M. At what temperature will the potential between the two electrodes be +0.140 V?