ZuoTi.Pro
Question

The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2...

The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures.

H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq)

The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures.

Pt(s) l Cr3+(aq), Cr2O72-(aq), H+(aq) ll H+(aq) l O2(g) l H2O(l) l Pt(s)

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2...
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

Similar Homework Help Questions

  • Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard...

    Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant Hg2+/Hg +0.85 F = 96485 C Fe3+/Fe2+ +0.77 2Fe3+(aq) + Hg(l) → 2Fe2+(aq) + Hg2+(aq) 2. The voltaic cell described by the balanced chemical equation has a standard emf of...

  • Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq)...

    Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq) + 14 H+ (aq) 6 I- (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) given that Cr2O72- = 1.7 M H+ = 1 M I- = 1 M Cr3+ = 0.002 M

  • 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 7.45×10-4 atm, the Cl- concentration is 1.21M, and the Cr3+ concentration is 1.37M ? 3Cl2(g) + 2Cr(s)6Cl-(aq) + 2Cr3+(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 the following...

  • For the electrochemical cell below, the half-cell on the left is the anode and the cell...

    For the electrochemical cell below, the half-cell on the left is the anode and the cell potential is 0.183 V at 25 °C. What is the concentration of H+, x, in mol L-1? Note: The symbol M is an abbreviation for mol L-1. Pt(s) | V2*(aq, 0.620 M), va(aq, 0.650 M) || H'(aq, xM) | H2(g, 1.30 bar) Pt(s) Half reaction 2 H(aq) 2eH2(g) V(a)V(aq) Eo V 0.000 -0.255 Enter a value accurate to 3 significant figures. x-[H]Number mol L-1

  • What is the calculated value of the cell potential at 298K for an electrochemical cell with the f...

    What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.62x10* atm, the F concentration is 1.18M, and the Cr3+concentration is 1.29M? 3F2(g) +2Cr(sF(aq) + 2Cr (aq) Answer:V The cell reaction as written above is spontaneous for the concentrations given: atm, What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 6.80x10...

  • 1) Balance the following reaction under acidic conditions and calculate the cell potential in (V) at...

    1) Balance the following reaction under acidic conditions and calculate the cell potential in (V) at 298 K generated by the cell. Report your answer to the hundredths place. Cr2O72-(aq) + I-(aq) → Cr3+(aq) + I2(s) [Cr2O72-] = 2.0 M, [H+] = 1.0 M, [I-] = 1.0 M, [Cr3+] = 1.0 × 10-5 M 2) What is the value of n for the following reaction? Enter the whole number. 3Ni+(aq) + Cr(OH)3(s) + 5OH-(aq) → 3Ni(s) + CrO42-(aq) + 4H2O(l)

  • 20;. The cell potential of the following electrochemical cell depends on the gold concentration in the...

    20;. The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s) | H2(g,1atm) | H+(aq,1.0M) | Au3+(aq,?M) | Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.22 V ? Express your answer using two significant figures. [Au3+]  = ______ M  

  • The cell potential of the following electrochemical cell depends on the gold concentration in the cathode...

    The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s)|H2(g,1atm)|H+(aq,1.0M)|Au3+(aq,?M)|Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.257 V ? Express your answer using three significant figures and in fM (f = femto = 10-15).

  • 1. Answer the following questions under standard conditions

    Ag3+(aq) + e− ⇌ Ag2+(aq)E° = 1.800 V2H+(aq) + 2e− ⇌ H2(g)E° = 0.000 V1. Answer the following questions under standard conditions(a) The half-cell containing Ag2+/Ag3+ is the cathode .(b) The half-cell containing H+/H2 is the anode .(c) What is E°cell (in V)? Report your answer to three decimal places in standard notation (i.e., 0.123 V).1.800 V(b) What is ΔG° (in kJ/mol) for the process that is occurring in the electrochemical cell? Report your answer to three significant figures in...

  • The cell potential of the following electrochemical cell depends on the gold concentration in the cathode...

    The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt($)|H2(9, 1.0 bar) H+ (aq, 1.0 mol L-Aus+ (aq,? mol L-)|Au(s). Part A What is the concentration of Au3+ in the solution if Ecell is 1.23 V ? Express your answer using two significant figures. YO ALC * * O O ? Au3+1 = mol L-1 Submit Request Answer

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
Active Questions
ADVERTISEMENT