Question 13; answer = -0.62 V
Question 14; answer= -2.048377 V
what are 13 and 14? Question 13 (5 points) For the following reaction: Cu(s) + Ni2+...
Conceptual: Consider a Sn(s)|Sn2+(aq) || Cu2+(aq)|Cu(s) cell. If the Sn2+ concentration is increased, what will happen to the measured Ecell value? • Calculation, full-reaction Nernst equation: Use the full Nernst equation to calculate Ecell for the conditions described… • Easier: Ni | Ni2+(0.300 M) || Cu2+(0.002 M) | Cu • Harder: Al | Al3+(0.002 M) || Cu2+(4.00 M) | Cu • Calculation, half-reaction Nernst equation: Use the Nernst equation to calculate E at pH 3.00 and [Cl- ] = 0.0035...
Consider the following reaction at 298K. Fe2+ (aq) + Ni (s) —> Fe (s) + Ni2+ (aq) Which of the following statements are correct? Choose all that apply. O K>1 delta Gº > 0 Bºcell > 0 The reaction is reactant-favored. n=2 mol electrons Submit Answer Retry Entire Group 6 m Consider the following reaction at 298K. Pb2+ (aq) + Cu(s) → Pb (s) + Cu2+ (aq) Which of the following statements are correct? Choose all that apply. Eºcell <...
QUESTION 4 Using the table below and the Nearnst Equation E-E° (0.0592/n)logQ Find the voltage of the cell: Cu2+(aq) + Ni(s) ? Cu(s) + Ni2+(aq) at 25° C if the concentrations of the soluble species are [Cu2+1-0.050 M and [Ni]- 1.40 M Reduction Reaction Sn2++ 2e-? Sn Cu2+ + 2e- ?Cu" Reduction Potential, Ecell 0.14 Volts 0.34 Volts 0.25 Volts +0.77 Volts Fe3+ + e-? Fe2+ 0.50 V 0.54 V 0.62 V 0.66 V
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
please show work and how they got this answer
12. Consider the cell reaction Cu(s) + 2Agt → Cu2+ + 2Ag(s). If [Ag+] = 1.0M and Ecell = 0.62 V, then what is the concentration of Cu2+7 Eºcell = +0.46 (0.80 -0.34), Q = x/1.02, x = [Cu2+] = 3.9x10-6
can you please help.me answer these three questions
please? I am really desperate and in need of help.
Question 7 Consider the following cell diagram: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s) Going from left to right represents the flow of charge, while || represents O positive, the salt bridge O negative, the salt bridge o positive, a phase boundary o negative, a phase boundary Question 8 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and Al3+ (aq)...
can you answer questions 7,8,9,10
Question 7 (10 points) ✓ Saved (7) For a galvanic cell notation: (-) Mg/Mg2+ (aq) // Cu2+ (aq) / Cu (+). which of the following is fully correct? (a) Mg2+ is oxidized to Mg, and Cu2+ (aq) is reduced to Cu O (b) Mg2+ is reduced to Mg, and Cu2+ (aq) is oxidized to Cu (c) Mg is oxidized to Mg2+, and Cu²+ (aq) is reduced to Cu (d) Mg is reduced to Mg2+, and...
please answer all wueston
Question 33 (3 points) (33) For a galvanic cell notation: (-) Ni /Ni2+ (aq) // Au3+ (aq) / Au (+), The electrode potentials: Eº (Ni2+/ Ni) = -0.257 V, E ° (AU3+ / Au ) = 1.498 V. The cell potential Eºcell (a) 1.241 V (b) - 1.755 V O (0) 1.755 V (d) 1.498 Why Question 35 (3 points) (35) For galvanic cell: (-) Cr/ Cr3+ (aq) / Cu2+ (aq) / Cu(+), the correct half...
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M and [Mn2+] = 0.30 M. 2 Al(s) + 3 Mn2+(aq) + 2 A13+(aq) + 3 Mn(s) Ecell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (cell) at 298 K. n= (Select] Q = (Select] Ecell = (Select)
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...