The two redox couples represented below are combined to create a galvanic cell. Which statements are true regarding this cell? Select all that apply. Br2(g) + 2 e – 2 Br (aq) Cr3+laq) + 3 e- E° = 1.087 V %3D > Cr(s) E° = -0.740 V Six electrons are transferred in the overall, balanced reaction for the cell. Cr(s) is the reducing agent. Cr3+ is reduced to Cr(s) at the cathode. Br2(g) is produced at the cathode. The overall, standard cell potential is 1.827 V Cr(s) is produced at the anode.

SOLVE STEP BY STEP DONT USE IA

Which of the following metals can be oxidized by H+ under standard conditions? Cu, Zn, Ag, Sn     Ag+(aq) + e– → Ag(s) E°  = 0.80 V   Cu2+(aq) + 2e– → Cu(s) E°  = 0.34 V   Cu2+(aq) + e– → Cu+(aq) E°  = 0.15 V   Sn4+(aq) + 2e– → Sn2+(aq) E°  = 0.13 V   Sn2+(aq) + 2e– → Sn(s) E°  = –0.14 V   Zn2+(aq) + 2e– → Zn(s) E°  = –0.76 V

For the galvanic (voltaic) cell 2+ - Fe(s) + Mn²+ (aq) → Fe²+ (aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²+] if [Mn²+] = 0.090 M and E = 0.78 V? Assume T is 298 K 1 4 7 +/- 2 LO 5 8 0.196 M 3 6 9 O X C x 100

Galvanic cell has 2 half reactions O2(g) + 4H+(aq) + 4e- → 2H2O(l)    E0red = +1.23 V            Cr3+(aq) + 3e- → Cr(s)         E0red = -0.74 V Write a balanced equation that describes the cell, ensuring that E0cell > 0 V and Calculate E0cell

The (fictional) metal unobtanium, Ub, has E° = −0.61 V for the reaction: Ub2+(aq) + 2 e− → Ub(s) a) If the galvanic cell shown below is spontaneous, which metal would be oxidized, and which would be reduced? How do you know? Support your answer with the half-reactions and E°cell. b) Write the overall reaction for this galvanic cell in cell notation.

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Ni

A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.

A galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)  Which of the following processes occurs at the cathode?    A. Cu(s) → Cu2+(aq) + 2e-   B. Cu2+(aq) + 2e-  → Cu(s)   C. Ag+(aq) + e-  → Ag(s)    D. Ag(s)  → Ag+(aq) + e-   E. Cu(s) + 2Ag+(aq)  → Cu2+(aq) + 2Ag(s)       Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     DOnt need work shown just answer asap        Predict the sign of ΔSorxn (positive or negative) for the following reactions:                                       CH3OH(l)  →  CH3OH(s)                                       CH4(g) + H2O(g)  →  CO(g) + 3…