Question

Given the measured cell potential, Ecell, is -0.3635 V at 25'C. In the following cell, calculate...

Given the measured cell potential, Ecell, is -0.3635 V at 25'C. In the following cell, calculate the H+ concentration.

Pt(s)/H2(g, 0.829 atm)/H+(aq, ?M)//Cd+2(aq,1.00M)/Cd(s)

The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E' are as followed.

2H+(aq)+2e- -> H2(g) E= 0.00V

Cd+2(aq) +2e- ->Cd(s) E= -0.403V

[H+]= ?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
A pH meter employs a voltaic cell for which the cell potential is very sensitive to...
A pH meter employs a voltaic cell for which the cell potential is very sensitive to pH. A simple (but impractical) pH meter can be constructed by using two hydrogen electrodes: one standard hydrogen electrode and a hydrogen electrode (with 1 atm pressure of H2 gas) dipped into the solution of unknown pH. The two half-cells are connected by a salt bridge or porous glass disk. a)Write the half-cell reactions for the cell. 1) No reaction. 2) H+(aq,1M)+H2O(l)→H3O+(aq), H2(g)→2H+(aq,1M)+2e−. 3)...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s)...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s) 0.337 2H+(aq)+2e−→H2(g) 0.000 A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.073 V at 298 K. Part A Based on the cell potential, what is the concentration of Cu2+ in this solution?...
The cell potential of the following electrochemical cell depends on the pH of the solution in...
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu2+(aq,1.0M)|Cu(s). What is the pH of the solution if Ecell is 360 mV ?
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2...
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e‐ → Zn(s) E° = ‐ 0.76 V Al3+(aq) + 3 e‐ → Al(s) E° = ‐ 1.66 V The standard potential for the galvanic cell that uses these two half-reactions is ________ V. 2)In the galvanic cell represented by the shorthand notation shown below, Cd(aq)|Cd2+(aq)|| I2(g)|I-(aq)|Pt(s) the inert electrode is ________, and the balanced cathode half-reaction reaction is ________.
A) What is the calculated value of the cell potential at 298K for an electrochemical cell...
A) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 8.15×10-4 atm, the Cl- concentration is 1.48M, and the Pb2+ concentration is 1.07M ? Cl2(g) + Pb(s) ---> 2Cl-(aq) + Pb2+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given:____ ( TRUE/FALSE ) B)What is the calculated value of the cell potential at 298K for an electrochemical cell with...
Exercise 18.46 Calculate the standard cell potential for each of the following electrochemical cells. Part A...
Exercise 18.46 Calculate the standard cell potential for each of the following electrochemical cells. Part A Ni2+(aq)+Mg(s)→Ni(s)+Mg2+(aq) Ecell=   V SubmitMy AnswersGive Up Part B 2H+(aq)+Fe(s)→H2(g)+Fe2+(aq) Express your answer using two significant figures. Ecell=   V SubmitMy AnswersGive Up Part C 2NO−3(aq)+8H+(aq)+3Cu(s)→2NO(g)+4H2O(l)+3Cu2+(aq) Express your answer using two significant figures. Ecell=   V
Exercise 20.105 Part A The cell potential of the following electrochemical cell depends on the pH...
Exercise 20.105 Part A The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu2+(aq,1.0M)|Cu(s). What is the pH of the solution if Ecell is 370 mV ? Express your answer using two significant figures. pH = SubmitMy AnswersGive Up
2. Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each...
2. Given the following pairs of half-reactions, please construct a complete balanced oxidation-reduction reaction for each pair of two half-reactions: (Show all work and steps) a)H2 →2H+ + 2e-    Fe2+ → Fe3+ + e- -------------------------------------------- b) 1/4O2 (g) + H+ + e- == ½ H2O H2 → 2H+ + 2e- -------------------------------------------- c) 2IO3- + 12H+ + 10e- == I2 + 6H2O 2I- = I2 + 2e-
1)A standard galvanic cell is constructed in which a H+ | H2 half cell acts as...
1)A standard galvanic cell is constructed in which a H+ | H2 half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) a) H2 is oxidized at the cathode. b) The cathode reaction is 2H+ + 2e- -> H2 c) Mn2+|Mn could be the other standard half cell. d) Fe3+|Fe2+ could be the other standard half cell. e) In the external circuit, electrons flow...
Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses...
Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses a basic electrolyte that has a 3.2 M hydroxide concentration. Cd(OH)2(s) + 2e- → Cd(s) + 2OH-(aq) Eº = -0.83 V NiO(OH)s) + H2O(l) + e- → Ni(OH)2(s) + OH-(aq) Eº = 0.52 V
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT