Question

Using standard electrode potentials calculate ΔG∘rxn and use its value to estimate the equilibrium constant for...

Using standard electrode potentials calculate ΔG∘rxn and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘C. Pb2+(aq)+Mg(s)→Pb(s)+Mg2+(aq).

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

from data table:

Eo(Mg2+/Mg(s)) = -2.372 V

Eo(Pb2+/Pb(s)) = -0.126 V

As per given reaction/cell notation,

cathode is (Pb2+/Pb(s))

anode is (Mg2+/Mg(s))

Eocell = Eocathode - Eoanode

= (-0.126) - (-2.372)

= 2.246 V

a)

number of electrons being transferred, n = 2

F = 96500.0 C

use:

ΔG = -n*F*E

= -2*96500.0*2.246

= -433478 J

= -433.5 KJ

Answer: -433.5 KJ

b)

here, number of electrons being transferred, n = 2

Eo = (2.303*R*T)/(n*F) log Kc

At 25 oC or 298 K, R*T/F = 0.0592

So, Eo = (0.0592/n)*log Kc

2.246 = (0.0592/2)*log Kc

log Kc = 75.8784

Kc = 7.558*10^75

Answer: 7.56*10^75

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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.
Use tabulated electrode potentials to calculate the equilibrium constant (K) at 25∘C for the following reaction....
Use tabulated electrode potentials to calculate the equilibrium constant (K) at 25∘C for the following reaction. Answer in units of x1017 Zn (s) + Ni2+ (aq) Zn2+ (aq) + Ni (s)
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox...
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb 2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard...
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) Fe2+(aq)+2e−→Fe(s) −0.45 Ni2+(aq)+2e−→Ni(s) −0.26
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
1. Calculate the equilibrium constant, K, for the reaction in the Galvanic Pb-Cu cell. (Report your...
1. Calculate the equilibrium constant, K, for the reaction in the Galvanic Pb-Cu cell. (Report your answer in scientific notation to three significant figures. Use * for the multiplication sign and ^ to designate the exponent.) Cu+ (aq) + Pb (s) → Cu (s) + Pb2+ (aq) Eocell = 0.647 V K = 2. For the reaction Mg (s) + Ni2+ (aq) →→ Mg2+ (aq) + Ni (s),    Eocell = 2.629 V.   Calculate the cell potential at T = 50.0oC...
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox...
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) ? 2 Fe3+(aq) + 6 I-(aq) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) 2 Fe3+(aq) + 6 I-(aq) 3.5 × 10-59 8.9 × 10-18 1.7 × 1029 6.1 × 1058 1.1 × 1017 Please explain with each every detail...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
From the standard reduction potentials listed in Table 7.1 for Sn2+|Sn and Pb2+|Pb, calculate the ratio...
From the standard reduction potentials listed in Table 7.1 for Sn2+|Sn and Pb2+|Pb, calculate the ratio of [Sn2+] to [Pb2+] at equilibrium at 25◦C and the ∆rG◦ value for the reaction.
Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant...
Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction: Co2+(aq) + 2Cu+(aq) Co(s) + 2Cu2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question. Equilibrium constant: G° for this reaction would be than zero.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT