Calculate the standard potential, E", for this reaction from its equilibrium constant at 298 K. X(s) + Y²+(aq) = X²+(aq)+Y(s) K = 1.67 × 10 %3D E = %3D
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Q: Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s)…
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Q: Calculate the standard potential, E, for this reaction from its equilibrium constant at 298 K. X(s)…
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Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
A: Given: X+3(aq) + e- ----> X+2 (aq) E°red = -0.69 V Y2(l) + 2e- -----> 2Y-(aq) E°red = -…
Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
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Q: Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s)…
A: The cell reaction is as follows: Xs +Y3+aq ⇔ X3+aq + Ys K = 5.32×10-7
Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
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A: Given Data:
Q: Calculate the standard potential, E, for this reaction from its equilibrium constant at 298 K. X(s)…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
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Q: The following reaction has an E value of -0.76 V: H2(g) + Zn2+(aq) -> Zn(s) + 2H+(aq) a. Calculate…
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Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
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Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
A: ΔG0=-nFE0cell E0cell = E0cathode - E0anode = -0.28 - ( -0.73) = 0.45 V
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A: Given values-> K = 8.99 × 10^-4
Q: Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K. X(s)…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
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Q: Calculate the standard free energy change in kJ given the standard reduction potentials for the half…
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Q: Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate…
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A: Answer :- 1.45 × 1012 The equilibrium constant (K) at 25°C for the given reaction = 1.45 × 1012…
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- V1 The biological standard reaction Gibbs energy of the reaction of removing phosphate from adenosine phosphate is -14 KJ/mol at 298 k and ph=7. What is the thermodynamic standard reaction Gibbs energy? AG= AG+ RTinQ = Use this equation to get lnQ. Please write down the detailsA) Calculate the standard reaction entropy at 298K of 1) Zn(s)+___Cu(aq) _____Zn(aq)+Cu (s) 2) C12H22O11(s)+12O2(g)____12CO2(g) + 11H2O(l) B) Continue the reaction entropies above with the reaction enthalpies, and calculate the standard reaction Gibbs energy at 298K. C) Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298K of the reactions above.From the biological standard half-cell potentialsE⊕(O2,H+,H2O) = +0.82 V and E⊕(NADH+,H+,NADH) = -0.32 V, calculate the standard potential arising from the reaction in which NADH is oxidized to NAD+ and the corresponding biological standard reaction Gibbs energy.
- The standard Gibbs energy of the reaction N2(g) + 3 H2(g) → 2 NH3(g) is −32.9 kJ mol−1 at 298 K. What is the value of ΔrG when Q = (i) 0.010, (ii) 1.0, (iii) 10.0, (iv) 100 000, (v) 1 000 000? Estimate (by interpolation) the value of K from the values you calculate. What is the actual value of K?Calculate the standard state AG for the following coupled reactions: A> B K'eq= 1.5 X 10S ×+Y= XY K'eq= 1.5 X 10-4 B+x+Y-A+XY AGO= ????Calculate the Free Gibb’s energy, kJ/mol, for a saturated solution of CdCO3 at 25.0°C. Ksp = 5.2 x 10-12
- The standard Gibbs energy of the reaction 2 NO2(g) → N2O4(g) is −4.73 kJ mol−1 at 298 K. What is the value of ΔrG when Q = (i) 0.10, (ii) 1.0, (iii) 10, (iv) 100? Estimate (by interpolation) the value of K from the values you calculate. What is the actual value of K?From information in the Resource section, calculate the standard Gibbs energy and the equilibrium constant at (i) 298 K and (ii) 400 K for the reaction PbO(s,red) + CO(g) ⇋ Pb(s) + CO2(g). Assume that the standard reaction enthalpy is independent of temperature.Construct a cycle similar to that in Fig. 3D.3 to analyse the reaction 1/2 H2(g) + 1/2 I2(s) → H+(aq) + I−(aq) and use it to find the value of the standard Gibbs energy of formation of I−(aq). You should refer to the tables in the Resource section for relevant values of the Gibbs energies of formation. As in the text, the standard Gibbs energy for the process H(g) → H+(g) + e−(g) should be approximated by the ionization energy, and that for I(g) + e−(g) → I−(g) by the electron affinity. The standard Gibbs energy of solvation of H+ can be taken as −1090 kJ mol−1 and of I− as −247 kJ mol−1.
- The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.Use standard Gibbs energies of formation to calculate the standard reaction Gibbs energies at 298 K of the reactions (i) Zn(s)+Cu2+(aq)→Zn2+(aq)+Cu(s) (ii)C12H22O11 (s)+12O2 (g)→12CO2(g)+11H2O(l)The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 Calculate the standard Gibbs energy of formation for A and B. Calculate the Gibbs energy change for the reaction A B at standard conditions. Calculate the enthalpy change for the reaction A à B at 350 K if the average heat capacity C0p = 42 J.K-1.mol-1.