Question

Use the following cell to answer the questions: Cr / Cr3+ (1.00 M) // Ni2+ (1.00...

Use the following cell to answer the questions:

Cr / Cr3+ (1.00 M) // Ni2+ (1.00 M) / Ni.

a) How many milligrams of Ni would be plated on the cathode if a current of 0.36 A is drawn for 3.5 hrs?

b) What is [Cr3+] when [Ni2+] has dropped to 10-4 M?

[Cr3+] =

c) What is the cell potential at the conditions described in Part b?

E =

Homework Answers

Answer #1

a) Mass of nickel plated on cathode (W) = Current X time X Eqt. Wt/96500

W = 0.36 X12600 X 29.35/96500 = 1.38g = 1380mg

b) The cell reaction is

2Cr(s) + 3Ni2+(aq) <------> 3Ni(s) + 2Cr3+(aq)

For every three moles of Ni2+ consumed 2 moles of Cr3+ are produced.

Moles of Ni2+ consumed = 1.0 - 10-4 = 0.9999

moles of Cr3+ formed = 2/3 X 0.9999 = 0.6666

therefore concentration of Cr3+ = 1.0 + 0.66666 = 1.6666

C) cell voltage at this concentration (E) = Eo - 0.0591log[Cr3+]/[Ni2+]

Eo = Eo cathode - Eo anode = -0.28 - (-0.74) = 0.46V

E = Eo - 0.0591log[1.6666]/[0.9999]

E = 0.46 - 0.0591log[1.6666]/[0.9999]

E = 0.448V

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
Use the following cell to answer the questions: Cr / Cr3+ (1.00 M) // Ni2+ (1.00...
Use the following cell to answer the questions: Cr / Cr3+ (1.00 M) // Ni2+ (1.00 M) / Ni. a) How many milligrams of Ni would be plated on the cathode if a current of 0.26 A is drawn for 1.5 hrs? mg Ni b) What is [Cr3+] when [Ni2+] has dropped to 10-4 M? [Cr3+] =  M c) What is the cell potential at the conditions described in Part b? E =  V
Use the following cell to answer the questions: Cr / Cr3+ (1.00 M) // Ni2+ (1.00...
Use the following cell to answer the questions: Cr / Cr3+ (1.00 M) // Ni2+ (1.00 M) / Ni. a) How many milligrams of Ni would be plated on the cathode if a current of 0.18 A is drawn for 2.9 hrs? mg Ni b) What is [Cr3+] when [Ni2+] has dropped to 10-4 M? [Cr3+] =  M c) What is the cell potential at the conditions described in Part b? E =  V
Consider a galvanic cell based upon the following half reactions: Ni2+ + 2e- → Ni -0.27...
Consider a galvanic cell based upon the following half reactions: Ni2+ + 2e- → Ni -0.27 V Cr3+ + 3e- → Cr -0.73 V How many of the following responses are true? 1. Adding equal amounts of water to both half reaction vessels will decrease the potential of the cell 2. Increasing the mass of the Ni will change the initial potential of the cell 3. Cr is being oxidized during the reaction 4. Decreasing the concentration of Ni2+ (assuming...
Ni(s) + 2 H+(? M) ----> Ni2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at...
Ni(s) + 2 H+(? M) ----> Ni2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.119 volts, what is the pH of the hydrogen electrode? pH =____
Calculate the Cd2+ concentration in the following cell if Ecell = 0.23 V. Cd(s)|Cd2+(x M)||Ni2+(1.00 M)|Ni...
Calculate the Cd2+ concentration in the following cell if Ecell = 0.23 V. Cd(s)|Cd2+(x M)||Ni2+(1.00 M)|Ni a. 0.0019 M b. 1.4 x 10-5 M c. 0.0036 M d. 0.015 M e. 0.0086 M
A voltaic cell utilizes the following reaction and operates at 298 K: 3Ce4+(aq)+Cr(s)→3Ce3+(aq)+Cr3+(aq). A) What is...
A voltaic cell utilizes the following reaction and operates at 298 K: 3Ce4+(aq)+Cr(s)→3Ce3+(aq)+Cr3+(aq). A) What is the emf of this cell under standard conditions? B) What is the emf of this cell when [Ce4+]= 2.4 M , [Ce3+]= 0.19 M , and [Cr3+]= 1.7×10−2 M ? C) What is the emf of the cell when [Ce4+]= 7.0×10−3 M ,[Ce3+]= 2.2 M , and [Cr3+]= 1.9 M ?
A voltaic cell contains two half-cells. One half-cell contains a nickel electrode immersed in a 1.00...
A voltaic cell contains two half-cells. One half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO3)2 solution. The second half-cell contains a titanium electrode immersed in a 1.00 MTi(NO3)3 solution. Ni2+(aq) + 2 e− → Ni(s)     E⁰red  = −0.257 V Ti3+(aq) + 3 e− → Ti(s)     E⁰red = −1.370 V (a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. ____V (b) Write the overall balanced equation for the voltaic cell....
A) A galvanic cell Zn(s)|Zn2+(aq) || Ni2+(aq)|Ni(s) is constructed using a completely immersed Zn electrode that...
A) A galvanic cell Zn(s)|Zn2+(aq) || Ni2+(aq)|Ni(s) is constructed using a completely immersed Zn electrode that weighs 43.2 g and a Ni electrode immersed in 503 mL of 1.00 M Ni2+(aq) solution. A steady current of 0.0555 A is drawn from the cell as the electrons move from the Zn electrode to the Ni electrode. Which reactant is the limiting reactant in this cell? Enter symbol ___________ How long does it take for the cell to be completely discharged? _____s...
The following cell has a potential of 0.040 V at 25°C. Zn(s)∣Zn2+(aq) || Cr3+(0.020 M) |...
The following cell has a potential of 0.040 V at 25°C. Zn(s)∣Zn2+(aq) || Cr3+(0.020 M) | Cr(s) What is the concentration of Zn2+? The standard reduction potentials are given below: Zn2+(aq) + 2e− → Zn(aq) Eo = − 0.760 Cr3+(aq) + 3e− → Cr(s) V Eo = − 0.740 V
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
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT