Question

For the following battery: Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s) a) Write the...

For the following battery: Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s)

a) Write the reduction half reaction occuring at the C(s) electrode. Include physical states of reactants and products

C(s) electrode: _____________________ Eo = 1.4V

b) From which electrode will electrons flow from the battery into a circuit? Cd(s) electrode or C(s) electrode

c) Calculate the mass of Cl2 consumed if the battery delivers a constant current of 783A for 48.0 min (in kg)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Cd(s) | CdCl2(aq) || Cl–(aq) | Cl2(l) | C(s)

a. reduction half reaction

Cl2 + 2e- ------> 2Cl-

b. Cd cell is oxidation half cell

Electrons are flow from Cd electrode to Cl2 half cell. Cd(s) electrode >>>>>>answer

c. Cl2 + 2e- ------> 2Cl-

W = MCt/ZF

Z = 2

M = 71g/mole

C = 783A

t   = 48min = 48*60 = 2880sec

W = MCt/ZF

W    = 71*783*2880/2*96500   = 829.6g    = 0.8296Kg >>>>answer

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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...
1)A voltaic cell is constructed in which the anode is a I-|I2 half cell and the...
1)A voltaic cell is constructed in which the anode is a I-|I2 half cell and the cathode is a Cl-|Cl2 half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external circuit, electrons migrate _____the I-|I2 electrode ____...
What are the products from the following single-replacement reaction? Cd(s) + AgNO3(aq) →
What are the products from the following single-replacement reaction? Cd(s) + AgNO3(aq) →
Consider the following reaction: 2 Na (s) + Cl2 (aq) ⟶ 2 NaCl (s) Which reactant...
Consider the following reaction: 2 Na (s) + Cl2 (aq) ⟶ 2 NaCl (s) Which reactant has been reduced? Which reactant has been oxidized? Determining masses of reactants and products mass of hydrate (CuSO4∙nH2O): _____________________ mass of anhydrous salt (CuSO4): _____________________ mass of water lost (H2O): _____________________ Determine the experimental mass percent of water in hydrate: mass % water = m (water lost) x100% =
The half-reactions that occur in ordinary alkaline batteries can be written as Cathode:MnO2(s)+H2O(l)+e−→MnO(OH)(s)+OH−(aq)Anode:Zn(s)+2OH−(aq)→Zn(OH)2(s)+2e− In 1999, researchers...
The half-reactions that occur in ordinary alkaline batteries can be written as Cathode:MnO2(s)+H2O(l)+e−→MnO(OH)(s)+OH−(aq)Anode:Zn(s)+2OH−(aq)→Zn(OH)2(s)+2e− In 1999, researchers in Israel reported a new type of alkaline battery, called a "super-iron" battery. This battery uses the same anode reaction as an ordinary alkaline battery but involves the reduction of FeO2−4 ion (from K2FeO4) to solid Fe(OH)3 at the cathode. Part A Use the following standard reduction potential and any data from Appendixes C and D to calculate the standard cell potential expected for...
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=?
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) O2(g) + Pb(s) → H2O(l) + Pb2+(aq) (b) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq) (c) Cl2(g) + Cr3+(aq) → Cl −(aq) + Cr2O72−(aq) (d) F2(g) + Mn2+(aq) → F −(aq) + MnO4−(aq)
Given: Cr3+(aq)+3e– ⇌Cr(s);E°=−0.74 V Cl2(g)+2e– ⇌2Cl−(aq);E°=1.36   What is the standard Gibbs free-energy change for the following...
Given: Cr3+(aq)+3e– ⇌Cr(s);E°=−0.74 V Cl2(g)+2e– ⇌2Cl−(aq);E°=1.36   What is the standard Gibbs free-energy change for the following reaction? (F = 96485 C per mole of electrons). 2Cr(s) +3Cl2(g) ⇔2Cr3+(aq) +6Cl−(aq) Select one: a. −1215 kJ b. −231.3 kJ c. −983 kJ d. −322.4 kJ e. 2309 kJ
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT