Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage...
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage developed by a cell consisting of Tl metal dipping in an aqueous solution that is 0.52 M in Tl+, connected by a porous bridge to a 0.56 M aqueous solution of HCl in contact with a Pt electrode over which H2 gas is bubbling at p = 0.85 bar. Please answer in volts.
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Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the
voltage...
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage...
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage developed by a cell consisting of Tl metal dipping in an aqueous solution that is 0.37M in Tl+, connected by a porous bridge to a 0.61 M aqueous solution of HCl in contact with a Pt electrode over which H2 gas is bubbling at p = 0.75 bar.
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage...
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage developed by a cell consisting of Tl metal dipping in an aqueous solution that is 0.59 M in Tl+, connected by a porous bridge to a 0.53 M aqueous solution of HCl in contact with a Pt electrode over which H2 gas is bubbling at p = 0.81 bar..
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage...
Given that Eo = -0.34 V for the reduction of Tl+ to Tl, find the voltage developed by a cell consisting of Tl metal dipping in an aqueous solution that is 0.58 M in Tl+, connected by a porous bridge to a 0.42 M aqueous solution of HCl in contact with a Pt electrode over which H2 gas is bubbling at p = 0.78 bar. V The number of significant digits is set to 2; the tolerance is +/-4%
Page 3 An electrochemical is prepared from a chromium metal electrode in contact solution of 0.500 M chromium (III)...
Page 3 An electrochemical is prepared from a chromium metal electrode in contact solution of 0.500 M chromium (III) nitrate and a standard hydrogen half-cell elect The two half cells are connected by a porous disk or a KCl salt bridge. Standard Reduction Potentials at 298 K Cr+ (aq) + 3e ----> Cr(s) Cr+ (aq) + e ----> Cr2+ (aq) E° = -0.740 V E° = -0.440 V a) Write the reaction for the cell and calculate the standard free...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
ALSO please find decomposition potential in V. Thank you! Standard Reduction Potentials (Volts) at 25 °C...
ALSO please find decomposition potential in V. Thank you!
Standard Reduction Potentials (Volts) at 25 °C I2 (s)+2 e>2 r(aq) 0.535 0 8)+4 H,o (a)+6 H,00) 1.229 2 H200)+2eH2g)+2 OH(aq) -0.828 -2.080 Se3+ (a)+3 eSe (s) A 0.189 M neutral aqueous Scl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials Half-reaction at anode: Half-reaction at cathode:
8-10 8. Determine the reduction potential for H2O(l) in neutral water: [H"]= [OH = 10? (6...
8-10
8. Determine the reduction potential for H2O(l) in neutral water: [H"]= [OH = 10? (6 points) (P. = 1 atm) 9. A cobalt electrode is placed in 1.00 L of I M CO(NO3)2(aq) and a chromium electrode is placed in 1.00 L of IM Cr(NO3)3(aq). Electrodes are connected by a wire through a voltmeter and the solutions are connected by a salt bridge. (16 points) a. The reduction reaction will be: b. The oxidation reaction will be: c. 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?...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
If a box is not needed, leave it blank Use the table Standard Reduction Potentials' located...
If a box is not needed, leave it blank Use the table Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur between Ni metal and C12(g), when the two are brought in contact via half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the productions are in aqueous solution. If no reaction will occur, leave all boxes blank. Submit Answer Retry Entire Group...
Page 3 An electrochemical is prepared from a chromium metal electrode in contact solution of 0.500 M chromium (III) nitrate and a standard hydrogen half-cell elect The two half cells are connected by a porous disk or a KCl salt bridge. Standard Reduction Potentials at 298 K Cr+ (aq) + 3e ----> Cr(s) Cr+ (aq) + e ----> Cr2+ (aq) E° = -0.740 V E° = -0.440 V a) Write the reaction for the cell and calculate the standard free...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
ALSO please find decomposition potential in V. Thank you!
Standard Reduction Potentials (Volts) at 25 °C I2 (s)+2 e>2 r(aq) 0.535 0 8)+4 H,o (a)+6 H,00) 1.229 2 H200)+2eH2g)+2 OH(aq) -0.828 -2.080 Se3+ (a)+3 eSe (s) A 0.189 M neutral aqueous Scl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials Half-reaction at anode: Half-reaction at cathode:
8-10
8. Determine the reduction potential for H2O(l) in neutral water: [H"]= [OH = 10? (6 points) (P. = 1 atm) 9. A cobalt electrode is placed in 1.00 L of I M CO(NO3)2(aq) and a chromium electrode is placed in 1.00 L of IM Cr(NO3)3(aq). Electrodes are connected by a wire through a voltmeter and the solutions are connected by a salt bridge. (16 points) a. The reduction reaction will be: b. The oxidation reaction will be: c. 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?...
If a box is not needed, leave it blank Use the table Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur between Ni metal and C12(g), when the two are brought in contact via half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the productions are in aqueous solution. If no reaction will occur, leave all boxes blank. Submit Answer Retry Entire Group...
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