Pd/Pd2+ (aq, 0.00010M)/ Br2 (l), Br-(aq, 0.00010M)/Pt(s) What is the Ecell?

Pd/Pd²⁺ (aq, 0.00010M)/ Br₂ (l), Br^-(aq, 0.00010M)/Pt(s)

What is the E_cell?

Expert Solution

Pb(s) ---------------> Pb^2+ (aq) + 2e^- E0 = 0.13v

Br2(l) + 2e^- ---------> 2Br^- (aq) E0 = 1.07v

---------------------------------------------------------------------------------------

Pb(s) + Br2(l) ------------> Pb^2+ (aq) + 2Br^-(aq) E0cell = 1.20v

n = 2

Ecell = E0cell- 0.0592/n logQ

= 1.20-0.0592/2 log[Br^-]^2[Pb^2+]

= 1.20-0.0296log(0.0001)^2*(0.0001)

= 1.20-0.0296log1*10^-12

= 1.20-0.0296*-12log10

= 1.20+0.3552

= 1.5552v >>>>answer

queen_honey_blossom answered 1 year ago

Balance the following redox reaction in acidic solution. Br? (aq) + MnO2 (s) ? Br2 (l)...

Balance the following redox reaction in acidic solution. Br? (aq) + MnO2 (s) ? Br2 (l) + Mn+2 (aq)

What is the standard Gibb’s Free Energy of the reaction graphite | Br-(aq) | Br2(l) |...

What is the standard Gibb’s Free Energy of the reaction graphite | Br-(aq) | Br2(l) | | I2(s) | I-(aq)? Is the reaction spontaneous under standard conditions? What is the initial cell potential of the voltaic cell represented by Zn | Zn+2 [0.100 M) | | Ni+2 (1.50 M) | Ni ? b. What is the cell potential when [Ni+]=0.500 M? c. What are the metal ion concentrations when the cell potential has fallen to 0.45 V?

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic?...

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic? A. -1.52V ; voltaic B. 1.52V ; electrolytic C. -1.52V ; electrolytic D. 1.52V ; voltaic

2Br–(aq) + 2H+(aq) + CO2(g) → Br2(aq) + HCOOH(aq) The concentration of the Br- falls from...

2Br–(aq) + 2H+(aq) + CO2(g) → Br2(aq) + HCOOH(aq) The concentration of the Br- falls from 0.120M to 0.080 M in 15 s. Calculate the amount of Br2(l) formed during the same time interval.

Consider the following reaction: Br2(l) + 2I-(aq) ---> 2Br-(aq) + I2(s) a.Calculate ΔGorxn b.Calculate K

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would...

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would be the value of K for AgBr(s) + 2NH3(aq) <--> Ag(NH3)2+(aq) + Br -(aq) ? b) What would be the molar solubility of silver bromide in 2.00 M aqueous ammonia?

BrO3- (aq) + 5Br- (aq) + 6H+ (aq) → 3Br2 (l) + 3H2O (l) [BrO3-]0 [Br-]0 [H+]0 ...

BrO3- (aq) + 5Br- (aq) + 6H+ (aq) → 3Br2 (l) + 3H2O (l) [BrO3-]0 [Br-]0 [H+]0 Initial Rate 0.100 0.100 0.100 8.00 E-4 0.200 0.100 0.100 1.60 E-3 0.200 0.200 0.100 3.20 E-3 0.100 0.100 0.200 8.00 E-4 1. what is the rate law? 2. what is the rate constant? 3. what is the overall order?

Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e-...

Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e- Al(s) -1.660V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Al(s) reduce Br2(l) to Br-(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank.

∆G for the reaction AgBr(s) ⇌ Ag+(aq) + Br- (aq) is 69.9 kj/mol at 25C. What...

∆G for the reaction AgBr(s) ⇌ Ag+(aq) + Br- (aq) is 69.9 kj/mol at 25C. What is the molar solubility of AgBr(s) at this temperature?

Question