Question

In: Chemistry

Use tabulated electrode potentials to calculate ΔG∘ for the reaction 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq)

Use tabulated electrode potentials to calculate ΔG∘ for the reaction 2K(s)+2H₂O(l)→H₂(g)+2OH⁻(aq)+2K⁺(aq)

Expert Solution

2K(s)+2H₂O(l) → H₂(g)+2OH⁻(aq)+2K⁺(aq)

The oxidation half cell reaction is : K(s) → K⁺(aq) + e^- ; E^o_K+/K = -2.925 V ---(1)

The reduction half cell reaction is : 2H₂O(l) + 2 e^- → H₂(g)+2OH^-(aq) ; E^o_2H+/H2 = -0.8277V ---(2)

Overall reaction is obtained as follows : [2xEqn(1)] + [Eqn(2)]

So standard potential of the cell , E^o = E^o_cathode - E^o_anode

= E^o_2H+/H2- E^o_K+/K

= -0.8277 - (-2.925) V

= +2.0973 V

We know that G^o = -nFE^o

Where

n = number of electrons transferred = 2

F = faraday = 96500 C

Plug the values we get G^o = -nFE^o

= -(2x96500x2.0973)

= -404.8x10³ J

= - 404.8 kJ

Therefore G^o = - 404.8 kJ

queen_honey_blossom answered 1 year ago

Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) Express your answer to three...

Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) Express your answer to three significant figures and include the appropriate units. ΔG∘ = nothing nothing Request Answer Part B Is the reaction spontaneous? Is the reaction spontaneous? no yes

For the following chemical reaction: Ba2+(aq) + 2OH-(aq) + H2O2(aq) + 2ClO2(aq) --> Ba(ClO2)2(s) + 2H2O(l)...

For the following chemical reaction: Ba2+(aq) + 2OH-(aq) + H2O2(aq) + 2ClO2(aq) --> Ba(ClO2)2(s) + 2H2O(l) + O2(g) a) Assign oxidation numbers to each element. b) State the elements undergoing oxidation. c) State the elements undergoing reduction. d) State the oxidizing agent. e) State the reducing agent. f) State the total number of electrons being transferred during the reaction.

Sodium and water react according to the reaction 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g) What...

Sodium and water react according to the reaction 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g) What number of moles of H2 will be produced when 4 mol Na is added to 2 mol H2O? a 1 mol b 2 mol c 3 mol d 4 mol e none of these Determine the limiting reactant when 4.00 mol of Sb are reacted with 5.00 mol Cl2 according to the unbalanced equation Sb + Cl2 ® SbCl3 a Sb b...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.

conc of oxalic acid: 0.7550M conc of MnO4=0.13M 3H2C2O4(aq) + 2MnO-4(aq)-------6CO2 (g)+2MnO2(s)+2OH- (aq)+2H2O(l) Experiment # H20...

conc of oxalic acid: 0.7550M conc of MnO4=0.13M 3H2C2O4(aq) + 2MnO-4(aq)-------6CO2 (g)+2MnO2(s)+2OH- (aq)+2H2O(l) Experiment # H20 Oxalic Acid KMnO4 1 6 5 1 2 1 10 1 3 5 5 2 Base on the equation and the reactants shown I need to determine: a)The initial concentration of each reactant. Show calculations b)final concentration of each reactance, considering: -which compound is the limiting reactant?Show calculations -which compound is in excess?Show calculations

Mg(s)+2H2O(l)→Mg(OH)2(s)+H2(g).Calculate the number of grams of Mg needed for this reaction to release enough energy to...

Mg(s)+2H2O(l)→Mg(OH)2(s)+H2(g).Calculate the number of grams of Mg needed for this reaction to release enough energy to increase the temperature of 75 mL of water from 21 ∘C to 76 ∘C. Calculate the standard enthalpy change for this reaction.

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

Using standard electrode potentials calculate ΔG∘ and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘C. Part A Cu2+(aq)+Zn(s)→Cu(s)+Zn2+(aq) USE ANY OF THESE VALUES Cu 2+ (aq) + e - ¡Cu^+ (aq) =0.16 e cell reduction Cu + (aq) + e - ¡ Cu(s) 0.52 ecell reduction potential Zn 2+ (aq) + 2 e - ¡ Zn(s) -0.76 cell reduction potential

Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C....

Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C. Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) Express the energy change in kilojoules to two significant figures. Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express the energy change in kilojoules to one significant figure. Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express the energy change in kilojoules to two significant figures.

Calculate ΔH°R for the reaction Mg(s) + 2H2O(l) → Mg(OH)2(s)+H2(g) at 350. K. Assume Cp,m does...

Calculate ΔH°R for the reaction Mg(s) + 2H2O(l) → Mg(OH)2(s)+H2(g) at 350. K. Assume Cp,m does not change with Temperature. How much did ΔH°R change from 298.15K to 350. 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.