14. This question has several parts that must be completed sequentially.DerivationDifferentiate the Lennard-Jones 6-12 potential equation (below) with respect to r to obtain an expression for o and ɛ. Express the equilibrium distance, re, in terms of o and show that V = -ɛ.V = 4ɛStep 1 of 3Differentiate the given equation with respect to r. (Use the following as necessary: ɛ, r, and o.)dVdrSubmit

When we differentiate a function with respect to specific term, then all other terms are considered…

Differentiate the Lennard-Jones 6-12 potential equation (below) with respect to r to obtain an expression for o and E. Express the equilibrium distance, re, in terms of o and show that V = -E. V = Step 1 of 3 Differentiate the given equation with respect to r. (Use the following as necessary: e, r, and o.) dv dr Submit

Differentiate the Lennard-Jones 6-12 potential equation (below) with respect to r to obtain an expression for o and E. Express the equilibrium distance, re, in terms of o and show that V = -E. V = Step 1 of 3 Differentiate the given equation with respect to r. (Use the following as necessary: e, r, and o.) dv dr Submit

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

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J R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H"(aq) + 4 e 2 H20 (1) 1.229 |Z2 (s) + 2 e → 2Z° (aq) 0.426 3+ (aq) + 3 е A' → A (s) 0.292 2 H20 (I) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 G2+ (aq) + 2 e G (s) - 1.245 (aq) + 2 e¯ → M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 MMZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 11 The electrode connected to the red wire (negative terminal on the battery) will... o produce bubbles and the pH will increase. o produce M (s) on the electrode and the pH will not change. o produce bubbles and the pH will decrease. o produce M (s) on the electrode and the pH will decrease. Question 12 The electrode…
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
Assignment 4 Consider the following dissociation reaction of iodine at 1000 K: 2(g) = 21(g) The following data is relevant: V(12) = 214.36 cm- %3D B(12)= 0.0373 cm-1 De(l2) = 1.5422 eV %3D The ground state of the iodine atoms is 2P3/2 which implies fourfold degeneracy. Calculate the equilibrium constant for the reaction. 13
6. When the ideal-gas reaction A+B=C+Dhas reached equilibrium, state whether or not each of the following relations must be true. Here n¡ is the number of moles of species i in equilibrium, P, is the partial pressure of i, and µ; is the chemical potential of i. Here a simple True or False answer is sufficient. (a) nc+np=nA +ng (b) Pc+Pp=PA+PB (c) na=ng (d) nc=na (e) If only A and B are present initially, then nc=np (f) Ha + HB= Hc+ Hp no matter what the initial composition. (g) If only A and B are present initially, then in equilibrium we must have nc # 0. (h) The equilibrium constant Kp(T)= PĄPB/(PcPp). (i) The value of –RT In Kp(T) = µE(T)+µ8(T)– H3(T) –- H§(T). ) The equilibrium constant is independent of the total pressure.
Given the dissociation reaction, Br2(g) = 2 Br(g), AH = + 112 kJ mol^ - 1 molecular bromine is 35 per cent dissociated at 1600 K and 1.00 bar at equilibrium. Calculate the equilibrium constant, K at 25\deg C. At what temperature would the reaction mixture need to be to turned off, ~ K = 10^-5?
A 25.00cm of potassium dichromate(K,Cr,CH so lution aretadded to an acidified aqueous solution of potassium lodide(present in excess). The lodine was then liberated according to the equation K-Cr.O;(aq) +14- (aq) + KI(ag) K(aq) + Cr (aq) + H;O(1) + 12(aq) Required 19.63cm of a 0.1478M Na S,O for complete reaction. The equation for the reaction of between Na S;03 and I2 is 2(aq)+ Na;S;SO;(aq)-Na S4O6(aq) + Nallac) Calculate the concentration of potassium dichromate (only 4 decimal places) mol/L
Calculate the value of Kc 2ClO3- + 12H+ +10e-←→Cl2 + 6H2O: E= +1.52 volt S2O82-+ 2e-←→ 2SO42-: E:+1.96 volt
Estimate the value of the equilibrium constant Kc for the reaction below from the data in the graph.
Q1: In argon gas, the interaction between two Ar atoms, separated by a distance r, can be very well described by the Lennard-Jones (LJ) potential energy: o12 V (r) = 4€ r12 76 The parameters o and e determine the shape and the strength of the potential. For argon, o = 0.34 nm and e = 120kg K (where kg is the Boltzmann constant). (a) Is the LJ interaction given above attractive or repulsive? What happens if two Ar atoms are brought very close to each other? What if they are far from each other? (b) Based on your answer in the previous part, describe the general motion of two Ar atoms brought close to each other and allowed to move from rest. (c) Does the LJ potential allow for equilibrium separation between two Ar atoms? If so, is it stable or unstable separation? (d) Based on your answers in the previous parts, determine the "spring constant" (in N/m) related to the LJ potential.
R = 8.314 mol·K F = 96, 485 moi AG = AG° + RT · In(Q) ΔΕΔΕ-().In(Q) RT Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 - Z2 (s) + 2 e 3+ (aq) + 3 e 2Z (aq) 0.426 → A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. If the A 3+ (aq) solution is diluted to 0.100 M and the G<* (aq) solution is diluted to 2+ 0.500 M, what is the initial value of Q under these new conditions? Report your answer with the correct significant figures.
(a) Complete the reaction scheme; what are the reagents labelled 1-7? +2 Et₂O PhMgBr (PhCH,)SnCl + 4 MeLi Đ 2 PhCH₂Cl + 2 Li(s) → 6 4 1. 3 2. H+ 7 5 Ph,COH + LiCl(s) (b) Describe the synthesis of UNSOLVATED Ph Al and Me.Si using fully balanced reaction equations describing all states of matter. (c) Describe and draw the solid state structures of UNSOLVATED Ph Al and Me.Si.
(2) The standard Gibbs energy, AG°, of the CH,OH CH,OPO,2- following reaction of rearrangement in aqueous H H H. H OH H но OH H но н он solutions at 20 °C is -7.1 kJ mol1. 0-PO,2- н он ÓH a. Calculate the equilibrium constant of this this Glucose-1-phosphate Glucose-6-phosphate reaction. Calculate the Gibbs energy of this reaction, AG, at concentrations of Glucose-1- b. phosphate, 0.01 mmol L-1 and of Glucose-6-phosphate, 0.01 mmol L-1 1 mmol L-1.