The electrical component of the Gibbs energy (i.e. the reversible electrical work) required to move an ion of charge Q=ze and radius R from a solvent with dielectric D₁ to a solvent with Q² dielectric D₂ is AGeler = Sxea R (1/2) W ▾ Part A Calculate AGelee if one mole of sodium ions is moved from air for which D₁=1.00 into water at T=300K. Note that between the temperatures of T=273K and T=373K the dielectric constant of water has the temperature dependence D₂ = 176 0.327() where T is the temperature in Kelvin units. Note: in the equation for the the dielectric constant of water the notation means you enter the numerical value for the temperature into the equation, but without the units K. Assume the radius of a sodium ion is R=2.00x10-10m. AGeler= -3.42×105 J Submit ✓ Correct Part B Previous Answers Calculate the entropy change A.Selec Submit ASelec= Value Part C μA Request Answer 8AC UT Units associated with the process described in Part A. ?

The electrical component of the Gibbs energy (i.e. the reversible electrical work) required to move an ion of charge Q=ze and radius R from a solvent with dielectric D₁ to a solvent with Q² dielectric D₂ is AGeler = Sxea R (1/2) W ▾ Part A Calculate AGelee if one mole of sodium ions is moved from air for which D₁=1.00 into water at T=300K. Note that between the temperatures of T=273K and T=373K the dielectric constant of water has the temperature dependence D₂ = 176 0.327() where T is the temperature in Kelvin units. Note: in the equation for the the dielectric constant of water the notation means you enter the numerical value for the temperature into the equation, but without the units K. Assume the radius of a sodium ion is R=2.00x10-10m. AGeler= -3.42×105 J Submit ✓ Correct Part B Previous Answers Calculate the entropy change A.Selec Submit ASelec= Value Part C μA Request Answer 8AC UT Units associated with the process described in Part A. ?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Here you are invited to explore the thermodynamic properties of a gas and its ability to condense to a liquid. Suppose that a gas obeys the van der Waals equation of state with the repulsive effects much greater than the attractive effects (that is, neglect the parameter a). (a) Find an expression for the change in molar Gibbs energy when the pressure is changed from pi to pf. (b) Is the change greater or smaller than for a perfect gas? (c) Estimate the percentage difference between the van der Waals and perfect gas calculations for carbon dioxide undergoing a change from 1.0 atm to 10.0 atm. (d) At the critical point of the gas, dp/dV = 0 and d2p/dV2 = 0. These relations identify the point of inflexion of the isotherms as shown. Show that a gas described by the equation of state p = nRT/V - an2/V2 + bn3/V3 shows critical behaviour, and express the critical constants in terms of the parameters a and b.
Estimate the vapour pressure of sea water at 20 °C given that the vapour pressure of pure water is 2.338 kPa at that temperature and the solute is largely Na+ and Cl- ions, each present at about 0.50 mol dm-3.
Calculate the standard Gibbs energy of the reaction CO(g) + CH3CH2OH(l) → CH3CH2COOH(l) at 298 K, using the values of standard entropies and enthalpies of formation given in the Resource section. The data for CH3CH2COOH(l) are ΔfH⦵ = −510 kJ mol−1, S⦵m = 191 J K−1 mol−1 at 298 K.
The standard Gibbs energy of formation of rhombic sulfur is zero and that of monoclinic sulfur is +0.33 kJ mol-1, at 25 °c.Which polymorph is the more stable at that 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.
What is the change in chemical potential of glucose when its concentration in water at 20.0 °c is changed from 0.10 mol dm-3 to 1.00 mol dm-3?
Calculate the standard Gibbs energy of reaction for 4 HI(g) + O2(g) → 2 I2(s) + 2 H2O(l) at 298 K, using the values of standard entropies and enthalpies of formation given in the Resource section.
By how much does the chemical potential of carbon dioxide at 310 K and 2.0 bar differ from its standard value at that temperature?
The excess Gibbs energy of a certain binary mixture is equal to gRTx(1 − x) where g is a constant and x is the mole fraction of a solute B. Find an expression for the chemical potential of B in the mixture and sketch its dependence on the composition.
Determine the (i) Gibbs energy, (ii) entropy, and (iii) enthalpy of mixing when 2.5 mol toluene is mixed with 2.5 mol of benzene at 298 K (assume an ideal solution)
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?
The standard molar entropies of water ice, liquid, and vapour at 298 K are 37.99, 69.91, and 188.83 J K-1 mol-1, respectively. On a single graph, show how the Gibbs energies of each of these phases vary with temperature; assume that the entropies themselves vary negligibly with temperature.