Balance the folllwng using half reaction method pls show all work and these equations are unbalanced
1. P4–>H2PO2-+PH3
Balance the folllwng using half reaction method pls show all work and these equations are unbalanced...
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) Cl– (aq) → ClO3– (aq) (ii) (acid solution) MoO3 (s) → Mo (s) (iii) (base solution) P4 (s) → H2PO2– (aq) (iv) (base solution) Se (s) → SeO32– (aq) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Show work please!
Balance the following redox reaction in acidic solution using the half reaction method. Show each step clearly and show all work so that partial credit can be given if needed. 3.
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3 – (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1.a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3– (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
Balance the Following Oxidation-Reduction reactions using the half-reaction method. Be sure to show your work. a) Xe + I2 = XeO3 + I^-1
3. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): Cr0(aq) + U" (aq) → Cr" (aq) +UO; (aq) (b) (acid solution): Cr(s) + O2(g) → Cr* (aq) (C) (basic solution): P. (s) + OH' (aq) → PH; (g) + H2PO2 (aq)
b) Balance the following reaction equations using the half-reaction method: 1. RCH2OH + H2Cro4 → RCO H 2. RCHO + Ag, HO/H,0 RCO, (-)
use the half reaction method to balance (SHOW ALL WORK) the following overall redox reaction describing the formation of acid mine drainage emanating from coal mines FeS2(s)+o2(g)+H2o(l)->FE(OH)3(s) +SO4 2-(aq) +H+(aq) balance redox entirely 1)FeS2+o2+h2o->fe2+ +So4 2- +h+ Balance redox entirely 2)2Fe2+ . + 1/2 O2 + 2H+ . ->2Fe3+ +H20 Balance this precipitation reaction Fe3+(aq) +3H2o(l) . -> F(OH)3 (s) +3H+(aq)
Determination of Oxalate in the Iron Oxalate Complex Use the half-reaction method to balance the titration equation in acid solution. (show work) D. MnOs + (unbalanced)
The following is an unbalanced redox reaction: Unbalanced Reaction: Al(s) + Co2+(aq) --> Al3+(aq) + Co(s) (a) Balance the above reaction using the half-reaction method. Show work. (b) The standard reduction potential for Al3+ to Al is ?red ° = −1.662 ? and the standard reduction potential for Co2+ to Co is ?red° = −0.277 V. Given this information, maximum amount of work, in kJ/mol rxn, for the balanced redox reaction from part (a) above. (T = 25.0 °C) Show...