both represent salt bridge.
using the standard reduction potential to find the E°cell. and to write the balanced reaction.
7) Write a balanced equation and determine Eº for each of the following cells: a) CrCr'|Ni?+|Ni...
QUESTIONS AND PROBLEMS Voltaic Cells 1. Write a balanced chemical equation for the overall cell reaction represented as a. (Pt) H2/H (Pt) Fe +/Fe2+ b. Cd/Cd2+ | Ni?+/Ni c. (PL) CI-/C1, | (Pt) MnO,-/Mn an aqueous gram of the Write the overall equa 6. Follow tl cell in which aqucous solt rrverale The
MnO−4 reacts with Fe2+ in acid solution to produce Fe3+ and Mn2+. Write a balanced equation for this reaction. Be sure to include the proper phases of matter in your response.
2) Day 18 & MQ16: Write the balanced net ionic equation for the following cells in acidic conditions: a. Cr(s) Cr" (aq) || Re" (aq)| Re(s) _Reacaq) +cres) _Rels) + _crofag) b. Pt() | H2O(1),02(g) || Cu?*(aq) Cu(s) - Ptest Cu 2+ cag) H2011) + Oziq) + Cu(s)
HELP NEED ANSWERED TODAY BY 11:50PM!!! Part A Write balanced equation for the anode of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Write balanced equation for the cathode of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express your answer as a chemical equation. Identify all of the phases in your answer. Part C Write balanced equation for overall cell reactions of the following galvanic cell Fe(s)|Fe2+(aq)||O2(g)|H+(aq),H2O(l)|Pt(s) Express...
Given the following line notation for an electrochemical cell, write the balanced net equation: Zn(s) | Zn2+ (aq, 1 M) || H+ (aq, 1 M), MnO4 - (1 M), Mn2+ (1 M) | Pt
17.32. Voltaic cells based on the following pairs of half-reactions are constructed. For each pair, write a balanced equation for the cell reaction, and identify which half-reaction takes place at each anode and cathode. a. Cdº'(aq) + 2 e - Cd(s) Agt(aq) + e - Ag(s) b. AgBr(s) + e - Ag(s) + Br"(aq) MnO2(s) + 4 H*(aq) + 2 e-Mn2(aq) + 2 H2O(0) c. PtCl 2- (aq) + 2 e-Pt(s) + 4 Cl(aq) AgCl(s) + e- Ag(s) + Cl(aq)
Given the following information: Ni2+ + 2e- Ni(s) Eº = -0.25 V Ag* + e. Ag(s) E° = 0.80 V 1) Determine the cell potential of the spontaneous redox reaction. 2) Give the net ionic equation for the overall balanced redox reaction. 3) Label the Galvanic Cell below to model the reaction above. Please include: • substances in each compartment • the salt bridge • the anode • the cathode 4) Give the line notation representation of this galvanic cell....
Write the balanced equation and calculate the E*cell for the following system: Fe(s) | Fe^2+(aq) | | Cr_2O_7^-(aq) | Cr^3+(aq) | Pt(s)
please answer in 10m
5. Balance each reaction, calculate the net Eº, and declare each reaction as being spontaneous or non- spontaneous. (9) a) Sn?' (aq) + Cr(s) → Sn(s) + Cr?" (aq) net Eº = b) Ag+ (aq) + Mn(s) Ag(s) + Mn2(aq) net Eº = c) Fe2(aq) + Cu(s) → Fe(s) + Cu?"(aq) net Eº =
2. Write the balanced equation, then determine the information requested in each of the following a. The number of moles and the mass of Mg required to react with 5.00 g of HCI and produce MgCl2 and H2. b. The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silvertl) oxide.