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4. Suppose that when the cell potential for the unknown solution in # 3 was measured,...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and...
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...
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for a...
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
A galvanic cell consists of a chromium anode immersed in a CrSO4 solution and a cobalt...
A galvanic cell consists of a chromium anode immersed in a CrSO4 solution and a cobalt cathode immersed in a CoSO, solution. A salt bridge connects the two half-cells (a) Write a balanced equation for the cell reaction. + (b) A current of 1.33 A is observed to flow for a period of 1.61 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? C mol (c) Calculate the...
Use the References to access important values if needed for this question. A student does an experiment to determine the molar solubility of lead chloride. He constructs a voltaic cell at 298 K consi...
Use the References to access important values if needed for this question. A student does an experiment to determine the molar solubility of lead chloride. He constructs a voltaic cell at 298 K consisting of a 0.709 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead chloride solution and a lead electrode in the anode compartment. If the cell potential is measured to be 4.96×10-2 V, what is the value of Ksp for...
4.In a electrochemical cell consisting of a silver electrode in a solution of AgNO3 and a...
4.In a electrochemical cell consisting of a silver electrode in a solution of AgNO3 and a gold electrode in a solution of Au(NO3)3 at standard conditions, the correct cell potential is 0.70 V b. 2.30 V 0.90 V d. -0.90 V 5. Predict which of the following reactions would exhibit an increase in entropy based on the nature of the reactants and products. 2H2(g) + O2(g) → 2H2O(g) 2NO2(g) → N2O4(g) H+(aq) + F-(aq) → HF(aq) BaF2(s) → Ba2+(aq) +...
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M...
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M solution of Pb(NO). In the second half-cell, solid germanium is in contact with a 1.00 M solution of Ge(NO), Ge is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 0.250 V at 25°C. (a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e'. Use the smallest integer...
The half cell voltage for a Fe^3+/Fe^2+ electrode is measured to be +0.810V. Based on this...
The half cell voltage for a Fe^3+/Fe^2+ electrode is measured to be +0.810V. Based on this information, and the E°red values provided, which species has a higher concentration? Fe^3+(aq) +e- --> Fe^2+(aq) E°red= 0.771V Fe^3+(aq) +3e- --> Fe(s) E°red= -0.037V Fe^3+(aq) +2e- --> Fe(s) E°red= -0.447V
Use the References to access important values if needed for this question An electrochemical cell consists...
Use the References to access important values if needed for this question An electrochemical cell consists of a Pt/H(aq,1.00 M) H (8) cathode connected to a Pt/H(aq)|Hz(8) anode in which the H concentration is that of a buffer consisting of a weak acid, HA(0.117 M), mixed with its conjugate base, A (0.193 M). The measured cell voltage is Ecell -0.169 V at 25 °C, with Pt. -1.00 atm at both electrodes. Calculate the pH in the buffer solution and the...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
i answered 0.58 but I got it wrong. can you help/solve? Question: A chemist measures the...
i
answered 0.58 but I got it wrong.
can you help/solve?
Question:
A chemist measures the potential of an electrochemical cell
vs. the saturated calomel electrode to be +0.5V. Then, the chemist
switches the reference electrode to the silver-silver chloride
electrode.
What should the voltage read?
Use the following diagram to assist your thought
process:
Previously we discussed a calomel reference electrode. A second type of reference electrode is also very common in lab - this one is called the...
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
A galvanic cell consists of a chromium anode immersed in a CrSO4 solution and a cobalt cathode immersed in a CoSO, solution. A salt bridge connects the two half-cells (a) Write a balanced equation for the cell reaction. + (b) A current of 1.33 A is observed to flow for a period of 1.61 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? C mol (c) Calculate the...
Use the References to access important values if needed for this question. A student does an experiment to determine the molar solubility of lead chloride. He constructs a voltaic cell at 298 K consisting of a 0.709 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead chloride solution and a lead electrode in the anode compartment. If the cell potential is measured to be 4.96×10-2 V, what is the value of Ksp for...
In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M solution of Pb(NO). In the second half-cell, solid germanium is in contact with a 1.00 M solution of Ge(NO), Ge is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 0.250 V at 25°C. (a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e'. Use the smallest integer...
Use the References to access important values if needed for this question An electrochemical cell consists of a Pt/H(aq,1.00 M) H (8) cathode connected to a Pt/H(aq)|Hz(8) anode in which the H concentration is that of a buffer consisting of a weak acid, HA(0.117 M), mixed with its conjugate base, A (0.193 M). The measured cell voltage is Ecell -0.169 V at 25 °C, with Pt. -1.00 atm at both electrodes. Calculate the pH in the buffer solution and the...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
i
answered 0.58 but I got it wrong.
can you help/solve?
Question:
A chemist measures the potential of an electrochemical cell
vs. the saturated calomel electrode to be +0.5V. Then, the chemist
switches the reference electrode to the silver-silver chloride
electrode.
What should the voltage read?
Use the following diagram to assist your thought
process:
Previously we discussed a calomel reference electrode. A second type of reference electrode is also very common in lab - this one is called the...
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