The standard molar entropy of Cl2 is 223.08 J - mol.K at P= 1.00 atm. For this molecule, i = 560 cm1, and the ground electronic state degeneracy is one. Using this information, determine the bond length of Cl2. Please explain the answer in detail.

The standard molar entropy of Cl2 is 223.08 J - mol.K at P= 1.00 atm. For this molecule, i = 560 cm1, and the ground electronic state degeneracy is one. Using this information, determine the bond length of Cl2. Please explain the answer in detail.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.9E

See similar textbooks

Similar questions

Derivation Calculate the entropy of HBr at 298 K and 1.00 bar, given that the bond length is 1.41 Å and the masses of ¹H and 79Br are 1.008 amu and 78.92 amu, respectively. The vibrational wavenumber is 2649 cm-¹. Step 1 of 7 Provide the equation needed to calculate the translational contribution to the total entropy. (Use the following as necessary: h, kB, m to represent the mass, P, T, and T.) (²³1) (2πmkT) h³ Strans = R In kµT (²/2) e P (2πmkBT) ³ kBT h³ P Step 2 of 7 Substitute numerical values into the equation from Step 1 to obtain a numerical calculation for the translational entropy contribution. Strans = 163.61 163.484901080763 J.K-1.mol-1 Step 3 of 7 Provide the equation needed to calculate the rotational contribution to the total entropy. (Use the following as necessary: h, I, kB, 7, σ, and T.) Srot = R In 8n²lkpT oh² + R 87² IkBT oh² Step 4 of 7 Substitute numerical values into the equation from Step 3 to obtain a numerical calculation for the rotational entropy…
Derivation Calculate the entropy of HBr at 298 K and 1.00 bar, given that the bond length is 1.41 Å and the masses of ¹H and 79Br are 1.008 amu and 78.92 amu, respectively. The vibrational wavenumber is 2649 cm-1. Step 1 of 7 Provide the equation needed to calculate the translational contribution to the total entropy. (Use the following as necessary: h, kB, m to represent the mass, P, π, and T.) (31) BT) = R In Strans (2μmk B¹ h³ KBT (2πmkBT) kBT P h³ P Step 2 of 7 Substitute numerical values into the equation from Step 1 to obtain a numerical calculation for the translational entropy contribution. XJ.K-1.mol-1 Strans =146.211 Submit
b. The standard molar entropy of O2 is 205.14 J mol-1 K-1 and v = 1580 cm-1 and the electronic ground state is triply degenerate. Determine the bond length of O2 from this information.
Determine the standard molar entropy of N2 (ν˜ = 2359 cm−1 , B = 2.00 cm−1 and electronic ground state has degeneracy 1 under standard thermodynamic conditions. You can assume ideal gas behaviour. 1. Calculate the standard internal molar energy U 2. Calculate the standard molar entropy S (standard thermodynamic conditions means T = 298 K and P = 1 atm.).
At what temperature is the standard molar entropy of helium equal to that of xenon at 298 K?
A certain molecule can exist in either a nondegenerate singlet state or a triplet state (with degeneracy of 3). The energy of the triplet exceeds that of the singlet by ε. When ?=??(where T is a set value, i.e., ? is a constant), calculate the values of the molecular partition function, molar heat capacity, and molar entropy. Assume the molecules are distinguishable and independent
Estimate the molar entropy of potassium chloride at 5 .0 K given that its molar heat capacity at that temperature is 1.2 mJ K-1 mol-1.
With a typical example, explain the concept of residual entropy
6.
The molar heat capacities for carbon dioxide at 298.0 K are shown below. C₁ = 28.95 J K-¹ mol-1 C₂ = 37.27 J K-¹ mol-1 The molar entropy of carbon dioxide gas at 298.0 K and 1.000 atm is 213.64 J K-1 mol-1. (a) Calculate the energy required to change the temperature of 1.000 mole of carbon dioxide gas from 298.0 K to 340.0 K, both at constant volume and at constant pressure. constant volume kJ kJ constant pressure (b) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.000 atm. JK-1 mol-1 (c) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.201 atm. JK-¹ mol-1
The molar heat capacities for carbon dioxide at 298.0 K are shown below. C = 28.95 J K-1 mol-1 Cp = 37.27 J K-1 mol-1 The molar entropy of carbon dioxide gas at 298.0 K and 1.000 atm is 213.64 J K-1 mol-¹. (a) Calculate the energy required to change the temperature of 1.000 mole of carbon dioxide gas from 298.0 K to 340.0 K, both at constant volume and at constant pressure. constant volume kJ constant pressure kJ (b) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.000 atm. JK-1 mol-1 (c) Calculate the molar entropy of CO₂(g) at 340.0 K and 1.139 atm. JK-1 mol-1
Calculate the molar entropy of a constant-volume sample of argon at 250 K given that it is 154.84 J K−1 mol−1 at 298 K; the molar constant-volume heat capacity of argon is 3/2 R.