Question

Given the following half reaction: Au^3+(aq) + 3e- ---> Au(s) Calculate the grams of Au produced...

Given the following half reaction: Au^3+(aq) + 3e- ---> Au(s) Calculate the grams of Au produced electrolyticaly using a current of 4.75 amps for 1 hour and 20 minutes.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) +...
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) + 2e- --> Cu(s) 0.342 V Ni2+(aq) + 2e- -->Ni(s) -0.257 V Calculate the potential at 25ºC for the following cell: Cu | Cu2+ [0.024M] || Ag+ [0.0048M] | Ag
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) -->...
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) --> Fe(s) + H3BO3(s) + 3H3O+(aq) The balanced reduction half-reactions for the above equation and their respective standard reduction potential values (E°) are as follows: Fe3+(aq) + 3e- --> Fe (s)... E=-0.04V H3BO3(s) + 3H3O+(aq) + 3e- ---> B(s)+6H20 (l).....E=-0.8698 K=?
Calculate the f.e.m. for the following reaction at 25oC Au3+(aq) (4.4e-3M) +   2Cl-(aq) (1.3e-2M)      →   Au(s)...
Calculate the f.e.m. for the following reaction at 25oC Au3+(aq) (4.4e-3M) +   2Cl-(aq) (1.3e-2M)      →   Au(s) ( - M) +   Cl2(g) ( - M) Ecell = ? (2 decimals accuracy!)
Given: Cr3+(aq)+3e– ⇌Cr(s);E°=−0.74V Sn4+(aq)+2e– ⇌Sn2+(aq);E°=0.15V What is the standard cell potential for the following reaction? 3Sn4+(aq)...
Given: Cr3+(aq)+3e– ⇌Cr(s);E°=−0.74V Sn4+(aq)+2e– ⇌Sn2+(aq);E°=0.15V What is the standard cell potential for the following reaction? 3Sn4+(aq) + 2Cr(s) ⇔3Sn2+(aq) + 2Cr3+(aq) Select one: a. 0.89 V b. −0.59 V c. 0.59 d. −0.89 V e. 0 V
Gold is produced electrochemically from a basic solution of Au(CN)6-1.Gold metal and O2(g) are produced at...
Gold is produced electrochemically from a basic solution of Au(CN)6-1.Gold metal and O2(g) are produced at the electrodes: Au(CN)6-1 + 3e à Au(s) + 6CN-1(aq) E0cell = 0.960 V O2(g) + 2 H2O + 4e à 4OH-1(aq) E0cell = 0.402 V 1) write the overall reaction (balanced net equation) 2) what volume of pure O2 is produced at 25 oC and 740 torr for every kilogram of Gold produced? {Use PV = nRT R = 0.0821 l.atm/mol.K }
Half-reaction E° (V) I2(s) + 2e- -----> 2I-(aq) 0.535V Cu2+(aq) + 2e- -----> Cu(s) 0.337V Cr3+(aq)...
Half-reaction E° (V) I2(s) + 2e- -----> 2I-(aq) 0.535V Cu2+(aq) + 2e- -----> Cu(s) 0.337V Cr3+(aq) + 3e- -----> Cr(s) -0.740V (1) The strongest oxidizing agent is: _____enter formula (2) The weakest oxidizing agent is: _____ (3) The weakest reducing agent is: _____ (4) The strongest reducing agent is: _____ (5) Will Cr3+(aq) oxidize I-(aq) to I2(s)? _____(yes)(no) (6) Which species can be reduced by Cu(s)? _____ If none, leave box blank.
A voltaic cell employs the reaction: 2Fe+3 (aq) + 3Mg (s) -> 2Fe (s) + 3Mg+2...
A voltaic cell employs the reaction: 2Fe+3 (aq) + 3Mg (s) -> 2Fe (s) + 3Mg+2 (aq) Calculate the Ecell at 25 degrees C under each of the following conditions. Fe+3 + 3e- -> Fe , Ered = -0.036 V 1. [Fe3+] = 1.00 M ; [Mg2+] = 1.00 M 2. [Fe3+] = 2.50 M ; [Mg2+] = 1.8x10-3 M Please show the work, thank you!
Given the cell reaction : 2 Cl – (aq) + Cu2+(aq)→ Cl2 (aq) + Cu (s)...
Given the cell reaction : 2 Cl – (aq) + Cu2+(aq)→ Cl2 (aq) + Cu (s) a) As written, is the cell galvanic or electrolytic? b) Calculate E°cell. c) Calculate ΔG°. 3. Using the standard reduction potentials given in Appendix of your text book, calculate the cell potential (E°cell ) at 298 K for each of the following reactions. (A) Br2 (aq) + 2 ClV (aq) → 2BrV (aq) + Cl2 (g) (B) A Galvanic Cell with the SHE and...
Given: Cr3+(aq)+3e−⇌Cr(s); E°=−0.74 V Pb2+(aq)+2e−⇌Pb(s); E°=−0.13  V What is the equilibrium constant (K) at  25°C  for...
Given: Cr3+(aq)+3e−⇌Cr(s); E°=−0.74 V Pb2+(aq)+2e−⇌Pb(s); E°=−0.13  V What is the equilibrium constant (K) at  25°C  for the following cell reaction? 2Cr(s)+3Pb2+(aq)→3Pb(s)+2Cr3+(aq) Select one: a. 7.4 ×10^61 b. 2.1×10^26 c. 2.9×10^44 d. 8.33x10^56
there are half reaction AgI(s) + e -⇌ Ag(s) + I-(aq) E° = -0.150 V Ag+(aq)...
there are half reaction AgI(s) + e -⇌ Ag(s) + I-(aq) E° = -0.150 V Ag+(aq) + e-⇌Ag (s) E° =0,80 V a) Calculate the standard potential of the reaction: AgI(s) + e - ⇌ Ag(s) + I-(aq)   b) Calculate the solubility product K(s) du AgI (s)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT