Consider the following reaction: MnO4 (ag) + 5FE2+ + 8H (aq) - Mn2+ (aq) + 5FE3+ (aq) + 4H2O) (aq) Initially the reaction is at standard conditions, and 298K. If the volume of the reservoir is 2.0L, what mass of NaOH (neglecting volume changes) is required to give a reduction potential of 0.55V? The reduction potential of MnO4 /Mn2* is 1.51V and that of Fe3+/Fe2* is 0.77V. O 79 g O 40 g O 58 g O 24 g O 93 g

Consider the following reaction: MnO4 (ag) + 5FE2+ + 8H (aq) - Mn2+ (aq) + 5FE3+ (aq) + 4H2O) (aq) Initially the reaction is at standard conditions, and 298K. If the volume of the reservoir is 2.0L, what mass of NaOH (neglecting volume changes) is required to give a reduction potential of 0.55V? The reduction potential of MnO4 /Mn2* is 1.51V and that of Fe3+/Fe2* is 0.77V. O 79 g O 40 g O 58 g O 24 g O 93 g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Provide clear handwriting and clear image
The standard reduction potential (E0cell= 0.54V) of reaction Br2 (l) + 2I (aq) > 2Br (aq) + I2 (s). What is the equilibrium constant at 25°C?
a) Balance the following reactions. b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. c) Identify the reactions with K > 1 among the following redox reactions. d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 + Br- --> Cl- + Br2 MnO4- + H+ + Ce3+ --> Ce4+ + Mn2+ + H2O Pb2+ -->Pb + Pb4+ NO3- + H+ + Zn --> Zn2+ + NO2 + H2O
Given the electrochemical cell described by: Mn(s)| Mn2+(aq)||Cr3+ (aq)| Cr(s) Calculate the cell potential at 250C if the concentration of Mn2+ (aq) is 0.800 M and the concentration of Cr3+ (aq) is 0.500 M. Report your answer to 3 significant figures. Use theStandard Reduction Potentials Table as needed. Ecell = V
Calculate values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) (a) Cr₂0₂2 (aq) + I¯(aq) = 1₂(s) + Cr³+ (aq) ४० spontaneity: (م) spontaneous not spontaneous balanced equation: chemPad XX→ ← (b) Cr₂0₂² (aq) + F¯(aq) = F₂(g) + Cr³+ (aq) 8⁰ V spontaneity: spontaneous not spontaneous balanced equation: chemPad XX Help H₂(g) → H+ (aq) + H(aq) Greek Help Greek
A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for 15.5 h. What mass of Mg is produced? g
Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
A student wanted to observe the reaction of Fe²+, (aq) V3+ (aq) Fe³+ (aq) + √2+ (aq) using an electrochemical cell. He did the setup and found out that the cell produced a voltage of -1.03V. Assuming standard conditions (298.15 K, 1 atm), which of the following observations would be correct? O a. The standard cell potential is equal to Eº v³+²+ - E°F 3+ Fe / Fe +2 3+ b. The reaction was spontaneous The reaction will proceed without any external power source O d. Exchanging the anode and cathode will make the voltage more negative
(a) What type of a battery is lead storage battery? Write the anode and cathode reactions and the overall cell reaction occurring in the operation of a lead storage battery.(b) Calculate the potential for half-cell containing 0.10 M K2Cr207(aq), 0.20 M Cr3+(aq) and 1.0 X 104M H+(aq)The half-cell reaction is K2Cr207–(aq) + 14 H+(aq) + 6e-2 ——–> 2Cr3+(aq) + 7H20(l) and the standard electrode potential is given as E°= 1.33 V.
Consider the following galvanic cell at 25°C. Pt | Cr²+ (0.25 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr²+ "(aq) + Co2+ Calculate the cell potential & for this galvanic cell and AG for the cell reaction at these conditions. + (aq) → 2 Cr³+ (aq) + Co(s) K = 2.79x107
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative