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.
Hydrogen peroxide (H2O2) is a possible product of the reduction of oxygen in acidic solution: 02(g)+2H+(aq) + 2 e-→ H2O2(,) H2O2(,) + 2 H+(aq) + 2 e-→ 2 H2O(aq) 02(g)+ 4 H+(aq)+4 e-→ 2 H20(,) E3 =0.70 V It can then be further reduced to water E2。 = 1.78 V The direct reduction of O2 to water has the following half-cell potential: E1 = 1.23 V (a) Compute ΔE° for the disproportionation of H2O2 in acidic solution. (b) Is H202...
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) • Observations · Evidence of the oxidation of Cr3+ • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction · Explain occurrence or non-occurrence of reaction by calculating cell. 2. Oxidation of H2O2: H2O2(aq) + FeCl3(aq) • Observations • Evidence of the oxidation of H2O2 • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction • Explain occurrence or...
For the voltaic cell shown, calculate the standard emf. Pt(s), H2(g) l H+(aq) ll H+(aq), H2O2(aq), H2O(l) l Pt(s) St. Red. Pot. (V) H+/H2 = 0 H2O2/H2O = 1.78
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)->H2O(1) + 12 02(g) is first order in H2O2- During one experiment it was found that when the initial concentration of 1,0, was 3.16x10-2 M, the concentration of H2O2 dropped to 8.09x10-3 M after 945 min had passed. Based on this experiment, the rate constant for the reaction is nin-1
8) AS is negative for the reaction A) C6H1206 (s) - 6C (s) + 6H2 (g)+302 (g) B) CH30H (I)-CH30H (g) C) Sr(NO3)2 (aq) 2LiOH (aq) Sr(OH)2 (s)+ 2LiNO3 (aq) D) LiOH (aq) Li+ (aq)+OH-(aq) E) 2H20 (g) 2H2 (g) 02 (8) (Sec. 19.4) 8) AS is negative for the reaction A) C6H1206 (s) - 6C (s) + 6H2 (g)+302 (g) B) CH30H (I)-CH30H (g) C) Sr(NO3)2 (aq) 2LiOH (aq) Sr(OH)2 (s)+ 2LiNO3 (aq) D) LiOH (aq) Li+ (aq)+OH-(aq) E)...
1) The reaction of hydrogen peroxide with iodine, H2O2(aq)+I2(aq)⇌OH−(aq)+HIO(aq) is first order in H2O2 and first order in I2. If the concentration of H2O2 was increased by half and the concentration of I2 was quadrupled, by what factor would the reaction rate increase? 2) Consider the following reaction: O3(g)→O2(g)+O(g) Using the results of the Arrhenius analysis (Ea=93.1kJ/mol and A=4.36×1011M⋅s−1), predict the rate constant at 298 K . 3. The rate constant of a chemical reaction increased from 0.100 s−1 to...
Reset Help S+02 - 02 Hg2/C_H403)2 + 2Naci - HgCl2 + 2NaCH:02 2KI + Pb(NO3)2 -- Pblz + 2KNO H2O2 + NaBr -NaBr + H20+02 Ba(NO3)2 + CuSO4 → BaSO4 + Cu(NO3)2 HCI + LiOH LiCl + H2O HBr + LiOH → LiBr + H2O Precipitation reactions Non-precipitation reactions
Which of the following are redox reactions? 2AgNO3(aq) + Cu(s) + Cu(NO3)2(aq) + 2Ag(s) 2Cus(s) + O2(g) + Cu(s) + SO2(g) 2AgNO3(aq) + Na2SO4(aq) + 2NaNO3(aq) + Ag2SO4(s) CO(g) + H2O(g) + CO2(g) + H2(g) CO2(g) + 2H20(1) + H30+(aq) + HCO3(aq)
7.40 Balance each of the following chemical equations: a. Zn(s) + HNO3(aq) H(g) + Zn(NO3)2(aq) b. Al(s) + H2SO4(aq) → H2(g) + Alz(SO2)3(aq) c. K SO,(aq) + BaCl(aq) → BaSO 9) + KCl(aq) d. CaCO3(s) — — Cao(s) + CO2(g) a. Zn(s) + HNO3(aq) —H2(g) + Zn(NO3)2(aq) b. Al(s) + H2SO4(aq) —> H2(g) + Al(SO4)3(aq) I
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Cr202-(aq) + NO2 (aq) = Cr3+ (aq) + NO3"(aq) Cr20,2- + NO3 + H+ + H2O= Cr3+ + NO3 + H+ + H20 (b) Mn04 (aq) + CH3OH(aq) Æ Mn2+ (aq) + HCO2H(aq) MnO4 + CH3OH + H+ + H2O= Mn2+ + HCO2H + H+ + H2O (c) ClO2(aq) + H2O2(aq) = C102 (aq) + O2(9) C102 + H2O2 + OH + H20 = ClO2...