When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of O2 is 2.21 atm, [K2Cr207] = 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(9) + Cr** (ag) → H2O2(ag) + Cr20,2 (ag) -2.51 O 2.70 -1.74 1.90 O 2.33 3.38 -3.12 O 2.92 O -3.51 -2.14 O O O O

When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of O2 is 2.21 atm, [K2Cr207] = 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(9) + Cr** (ag) → H2O2(ag) + Cr20,2 (ag) -2.51 O 2.70 -1.74 1.90 O 2.33 3.38 -3.12 O 2.92 O -3.51 -2.14 O O O O

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

Write equations for the oxidation and reduction half-reactions and the net reaction describing the displace of Cu 2+(aq) by Fe (s) the oxidation of Br – to Br2 (aq) by Cl(aq) the reduction of Fe3+(aq) + (to Fe2+(aq) + by Al(s)) the oxidation of Cl –(aq) + ClO3- (aq) by MnO4- in acidic solution
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)
Complete and balance the following redox reaction in basic solution Cr.0, (aq) + 1,(s) Cr (aq) + 10, (aq) 口4|□ O2. O+02+ O 3+ 04+ 3 4 7 8 O2 03 04 Os 06 0708O9 0. (s) (1) (g) (aq) -> e OH Cr H,O H,O* Reset æ H,O Delete LO 2.
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)
Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V
K124.
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V
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
A galvanic cell is constructed in which the overall reac- tion is Cr,O} (aq) + 14 H¿O*(aq) + 6 I (aq) → 2 Cr* (aq) 1 3 I,(s) | 21 H,0(€) (a) Calculate AE° for this cell. (b) At pH 0, with [C»O3¯] = 1.5 M and [I-] = 0.40 M, the cell potential is found to equal 0.87 V. Calculate the concentration of Cr³*(aq) in the cell.
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V
Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀ Ti2+(aq)+Co(s) occurs at 25 °C, given that [Ti2 + ] = 0.00180 M and [Co2 + ] = 0.813 M. Refer to the table of standard reduction potentials.