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5. In aqueous solution Cutions are more stable than Cu ions because 2 Cut...
5. In aqueous solution Cuions are more stable than Cu ions because 2 Cu" (aq) +...
5. In aqueous solution Cuions are more stable than Cu ions because 2 Cu" (aq) + Cu (aq) + Cu(s) (a) Give an oxidation hall-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for the reaction. (1 mark) 6. Refer to Fig. 1. The salt bridge is to prevent wholesale mixing of the two solutions. Assume that...
Equation 18: (didnt mean to attach equation 15 oops) V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE...
Equation 18: (didnt mean to attach equation 15 oops)
V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 5. In aqueous solution Cu* ions are more stable than Cu ions because 2 Cu* (aq) + Cu2+ (aq) + Cu (s) (a) Give an oxidation half-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for...
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for...
In step1, aqueous ammonia is added to a solution of the three ions. The equilibrium for the ammonia is EQ1: NH3(aq + H2O(l) ßà NH4+(aq) Kb=1.8x10-5 The bismuth(III) ion is precipitated out of the solution as Bi(OH)3. The equilibrium involved is related to the one provided below: EQ2: Bi(OH)3(s) ßà Bi3+(aq) +3OH(aq)- Ksp =3.2x10-40 Manipulate EQ 1 and 2 to solve for the net equation, EQ3: EQ3 (net): 3H2O+ Bi3+(aq) +3NH3(aq) ßàBi(OH)-(s) +3NH4+(aq) Write the mass law expression for the...
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and...
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and Ag+ ions setting up a corrosion cell. a) Show the anode and cathode reactions. b) Now show the overall cell reaction. c) If [Cu2+] = 10-M and (Ag*] -0.5M, calculate the cell voltage. Except for sign, standard electrode potentials are absolute. They do not change if you change the stoichiometry of the reaction. Electrode Reaction E° (V) Cu2+ + 2e = Cu Ag+ +e...
2 A voltaic cell is set up with one beaker containing 1.0 M Cu(NO 3) 2...
2 A voltaic cell is set up with one beaker containing 1.0 M Cu(NO 3) 2 and a copper electrode, and another beaker containing 1.0 M Mn(NO 3) and a manganese electrode. Given the following standard reduction potentials, answer the 3 questions below: E Cu2+(aq) + 2e Cu(s) 0.34 V Mn2+(aq) + 2e + Mn(s) 1.18V Part a. Write out the half-cell reaction that occurs at the anode of the voltaic cell. Part b. In which direction do electrons flow?...
Copper(I) ions in aqueous solution react with NH, (aq) according to Cut (aq) + 2 NH,...
Copper(I) ions in aqueous solution react with NH, (aq) according to Cut (aq) + 2 NH, (aq) + Cu(NH2) (aq) K = 6.3 x 1010 Calculate the solubility (in g.L-) of CuBr(s) (Kyp = 6.3 x 10') in 0.14 M NH3(aq). solubility of CuBr(s):
with the information and tables provided, can you help me answer questions 2,3,4,and 5? thank you!...
with the information and tables provided, can you help me
answer questions 2,3,4,and 5? thank you!
DATA ANALYSIS - ONLINE SIMULATION DATA Record your collected data here. Black Red E (V) Cu Zn -1.10 Cu Sn -0.48 Cu Mg -2.71 Cu Ag 0.46 QUALITY OF DATA This section awards marks based on the quality of your Ell values. Quality of data Your standard cell potentials are in the expected order. EXPECTED DATA The expected data is given below. Use the...
Copper(I) ions in aqueous solution react with NH3(aq) according to Cut(aq)2 NH (aq) - Cu(NH(aq) =...
Copper(I) ions in aqueous solution react with NH3(aq) according to Cut(aq)2 NH (aq) - Cu(NH(aq) = 6.3 x 1010 Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 x 109) in 0.64 M NH3 (aq) solubility of CuBr(s): g/L
*A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the ce...
*A copper, Cu(s), electrode is immersed in a solution that is
1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II),
[Cu(NH3)4]2+. If a standard hydrogen electrode is used as the
cathode, the cell potential, Ecell, is found to be 0.070 V at 298
K.
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [NH. If a standard hydrogen electrode is used as the cathode, the cell potential,...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3,...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(I), [Cu(NH). If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.074 V at 298 K Constants Periodic Table Use the standard reduction potentials shown here to answer the questions Reduction half-reaction E (V) Cu2+ (aq) 2e Cu(s) 0.337 2H + (aq) + 2e →H, (g) | 0.000 ▼ Part A...
5. In aqueous solution Cuions are more stable than Cu ions because 2 Cu" (aq) + Cu (aq) + Cu(s) (a) Give an oxidation hall-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for the reaction. (1 mark) 6. Refer to Fig. 1. The salt bridge is to prevent wholesale mixing of the two solutions. Assume that...
Equation 18: (didnt mean to attach equation 15 oops)
V-13 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 5. In aqueous solution Cu* ions are more stable than Cu ions because 2 Cu* (aq) + Cu2+ (aq) + Cu (s) (a) Give an oxidation half-cell reaction and a reduction half-cell reaction that can be combined to form this overall reaction. (0.5 marks) (b) Use Eq. 18 with your answer to (a) to calculate the theoretical K for...
9. Copper and silver are in contact with an aqueous solution at 25°C containing Cu2+ and Ag+ ions setting up a corrosion cell. a) Show the anode and cathode reactions. b) Now show the overall cell reaction. c) If [Cu2+] = 10-M and (Ag*] -0.5M, calculate the cell voltage. Except for sign, standard electrode potentials are absolute. They do not change if you change the stoichiometry of the reaction. Electrode Reaction E° (V) Cu2+ + 2e = Cu Ag+ +e...
2 A voltaic cell is set up with one beaker containing 1.0 M Cu(NO 3) 2 and a copper electrode, and another beaker containing 1.0 M Mn(NO 3) and a manganese electrode. Given the following standard reduction potentials, answer the 3 questions below: E Cu2+(aq) + 2e Cu(s) 0.34 V Mn2+(aq) + 2e + Mn(s) 1.18V Part a. Write out the half-cell reaction that occurs at the anode of the voltaic cell. Part b. In which direction do electrons flow?...
Copper(I) ions in aqueous solution react with NH, (aq) according to Cut (aq) + 2 NH, (aq) + Cu(NH2) (aq) K = 6.3 x 1010 Calculate the solubility (in g.L-) of CuBr(s) (Kyp = 6.3 x 10') in 0.14 M NH3(aq). solubility of CuBr(s):
with the information and tables provided, can you help me
answer questions 2,3,4,and 5? thank you!
DATA ANALYSIS - ONLINE SIMULATION DATA Record your collected data here. Black Red E (V) Cu Zn -1.10 Cu Sn -0.48 Cu Mg -2.71 Cu Ag 0.46 QUALITY OF DATA This section awards marks based on the quality of your Ell values. Quality of data Your standard cell potentials are in the expected order. EXPECTED DATA The expected data is given below. Use the...
Copper(I) ions in aqueous solution react with NH3(aq) according to Cut(aq)2 NH (aq) - Cu(NH(aq) = 6.3 x 1010 Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 x 109) in 0.64 M NH3 (aq) solubility of CuBr(s): g/L
*A copper, Cu(s), electrode is immersed in a solution that is
1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II),
[Cu(NH3)4]2+. If a standard hydrogen electrode is used as the
cathode, the cell potential, Ecell, is found to be 0.070 V at 298
K.
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [NH. If a standard hydrogen electrode is used as the cathode, the cell potential,...
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(I), [Cu(NH). If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.074 V at 298 K Constants Periodic Table Use the standard reduction potentials shown here to answer the questions Reduction half-reaction E (V) Cu2+ (aq) 2e Cu(s) 0.337 2H + (aq) + 2e →H, (g) | 0.000 ▼ Part A...
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