Question

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br– (aq) + I2(s) Br2(l) +...

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br– (aq) + I2(s) Br2(l) + 2I– (aq)

5.7 ? 10–19 is the correct answer

Can someone explain how they got this answer

Homework Answers

Answer #1

The reaction

    2Br - (aq) + I2 (s) Br2(l) + 2I - (aq)

The standard reduction potentials of the half-cell reactions are followings

Br2 (l) + 2e- 2Br-(aq) E0 = +1.07V

I2(s) + 2e- 2I -(aq)    E°= +0.53V

Overall

2Br - (aq) + I2 (s) Br2(l) + 2I - (aq)

We know,

E0cell   =  E0cathode - E0anode
E0cell = +0.53V - 1.07V

E0cell = -0.54V

We know

E0cell = (0.0592/n) log K (K is the equilibrium constant)

log K = (-0.54*2)/(0.0592)

K = 5.7 *10-19(Answer)

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
for the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C....
for the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C. Determine the initial and equilibrium concentrations of Br if the initial and equilibrium concentrations of Br2 are 5.70 ×10−3 M and 5.30 × 10−3M, respectively.
Calculate the equilibrium constant for each of the reactions at 25 ?C. Standard Electrode Potentials at...
Calculate the equilibrium constant for each of the reactions at 25 ?C. Standard Electrode Potentials at 25 ?C Reduction Half-Reaction E?(V) Pb2+(aq)+2e? ?Pb(s) -0.13 Mg2+(aq)+2e? ?Mg(s) -2.37 Br2(l)+2e? ?2Br?(aq) 1.09 Cl2(g)+2e? ?2Cl?(aq) 1.36 MnO2(s)+4H+(aq)+2e? ?Mn2+(aq)+2H2O(l) 1.21 Cu2+(aq)+2e? ?Cu(s) 0.16 Part A: Pb2+(aq)+Mg(s)?Pb(s)+Mg2+(aq) Express your answer using three significant figures. Part B: Br2(l)+2Cl?(aq)?2Br?(aq)+Cl2(g) Express your answer using two significant figures. Part C: MnO2(s)+4H+(aq)+Cu(s)?Mn2+(aq)+2H2O(l)+Cu2+(aq) Express your answer using two significant figures.
Write the equilibrium‑constant expression for the reaction A(s)+3B(l)↽−−⇀2C(aq)+D(aq)A(s)+3B(l)↽−−⇀2C(aq)+D(aq) in terms of [A],[A], [B],[B], [C],[C], and [D],[D],...
Write the equilibrium‑constant expression for the reaction A(s)+3B(l)↽−−⇀2C(aq)+D(aq)A(s)+3B(l)↽−−⇀2C(aq)+D(aq) in terms of [A],[A], [B],[B], [C],[C], and [D],[D], as needed. Note that ?c,Kc, which is sometimes symbolized as ?eq,Keq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, ?cKc means the same thing as ?eq.
1. Calculate the equilibrium constant Keq for the following reaction at 25°C: 3Fe2+(aq) + 2Cr(s) ↔...
1. Calculate the equilibrium constant Keq for the following reaction at 25°C: 3Fe2+(aq) + 2Cr(s) ↔ 3Fe(s) + 2Cr3+(aq) 3.8 x 10–31 7.2 x 10–11 1.4 x 1010 2.6 x 1030 1.6 x 1015 2. A 1M aqueous solution of copper(II) nitrate is electrolyzed. What are the predicted products at the anode and cathode? N2 gas at the anode; copper metal at the cathode O2 gas at the anode; copper metal at the cathode NO2 gas at the anode; copper...
Consider the reaction CaSO4(s)⇌Ca2+(aq)+SO2−4(aq) At 25 ∘C the equilibrium constant is Kc=2.4×10−5 for this reaction. If...
Consider the reaction CaSO4(s)⇌Ca2+(aq)+SO2−4(aq) At 25 ∘C the equilibrium constant is Kc=2.4×10−5 for this reaction. If the resulting solution has a volume of 1.1 L , what is the minimum mass of CaSO4(s) needed to achieve equilibrium? Express your answer to two significant figures and include the appropriate units.
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) -->...
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) --> Fe(s) + H3BO3(s) + 3H3O+(aq) The balanced reduction half-reactions for the above equation and their respective standard reduction potential values (E°) are as follows: Fe3+(aq) + 3e- --> Fe (s)... E=-0.04V H3BO3(s) + 3H3O+(aq) + 3e- ---> B(s)+6H20 (l).....E=-0.8698 K=?
Determine the equilibrium constant for the following reaction         X(OH)2(s) + 2 H+(aq) = X2+(aq) +...
Determine the equilibrium constant for the following reaction         X(OH)2(s) + 2 H+(aq) = X2+(aq) + 2 H2O(l) given the chemical reactions below. X(OH)2(s) = X2+(aq) + 2 OH–(aq) K = 3 x 10–10 H2O(l) = H+(aq) + OH–(aq) K = 1.0 x 10–14
Compute the equilibrium constant at 25 ∘ C for the reaction between Fe 2+ (aq) and...
Compute the equilibrium constant at 25 ∘ C for the reaction between Fe 2+ (aq) and Zn(s) which form Fe(s) and Zn 2+ (aq)
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s) Standard Reduction Potentials...
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s) Standard Reduction Potentials at 25 ∘C Fe2+(aq)+2e−→Fe(s) E∘= −0.45 V Ag+(aq)+e−→Ag(s) E∘= 0.80 V
Calculate the equilibrium constant Keq for the following reaction at 25°C. (S° values in J/mol•K: N2(g),...
Calculate the equilibrium constant Keq for the following reaction at 25°C. (S° values in J/mol•K: N2(g), 191.5 ; O2(g), 205.0 ; Cl2(g), 223.0 ; NOCl(g), 261.6) N2(g) + O2(g) + Cl2(g) ↔ 2NOCl(g) ΔH° = 103.4 kJ a. 2.43 x 10−20 b. 8.82 x 10−29 c. 5.91 x 10−17 d. 2.01 x 10−10 e. 6.99 x 10−24