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Problem 3) Take the creation of salt from sodium and molecular chlorine: 2 Na + C12 =2 NaCl A) Write out how the equilibrium constant K will be related to the concentrations of each chemical (as variables, similar to eqn: [H2][H]- : [H2] = K(t)). [H]2 %3D B) Write out what the equilibrium constant K will be from the quantum concentrations and internal free energy of each molecule (as variables, similar to eqn: log K = log ng(H2) – 2 log no(H) – 2) %3D C) Find the exact numerical equilibrium constant if the internal free energies are equal to the dissociation energies (FNa = 0, FNaci = -4.26 eV, and Fci = -2.48 eV), and the masses are m2 MNaci = 6.0 × 10-7eVs² of the system is . A useful constant is T = 300k = 0.26 eV. Mclz , MNa = 2.3 x 10-7 eVs² m2 = 7.3 x 10-7 eVs² ,and the temperature %3D m2 A useful constant is h = 6.58 × 10-16 eVs D) Finally, use the equilibrium constant to find how many moles of NaCl will exist in equilibrium with 1.0 mole of Na and 1.0 mole of Cl2.

Problem 3) Take the creation of salt from sodium and molecular chlorine: 2 Na + C12 =2 NaCl A) Write out how the equilibrium constant K will be related to the concentrations of each chemical (as variables, similar to eqn: [H2][H]- : [H2] = K(t)). [H]2 %3D B) Write out what the equilibrium constant K will be from the quantum concentrations and internal free energy of each molecule (as variables, similar to eqn: log K = log ng(H2) – 2 log no(H) – 2) %3D C) Find the exact numerical equilibrium constant if the internal free energies are equal to the dissociation energies (FNa = 0, FNaci = -4.26 eV, and Fci = -2.48 eV), and the masses are m2 MNaci = 6.0 × 10-7eVs² of the system is . A useful constant is T = 300k = 0.26 eV. Mclz , MNa = 2.3 x 10-7 eVs² m2 = 7.3 x 10-7 eVs² ,and the temperature %3D m2 A useful constant is h = 6.58 × 10-16 eVs D) Finally, use the equilibrium constant to find how many moles of NaCl will exist in equilibrium with 1.0 mole of Na and 1.0 mole of Cl2.

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
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Problem 3) Take the creation of salt from sodium and molecular chlorine: 2 Na + C12 =2 NaCl A) Write out how the equilibrium constant K will be related to the concentrations of each chemical (as variables, similar to eqn: [H2][H]-2 [H2] = K(t)). [H]2 %3D B) Write out what the equilibrium constant K will be from the quantum concentrations and internal free energy of each molecule (as variables, similar to eqn: log K = log no (H2) – 2 log no (H) - ) %3D C) Find the exact numerical equilibrium constant if the internal free energies are equal to the dissociation energies (FNa = 0, FNaci = -4.26 eV, and Fci = -2.48 e), and the masses are = 7.3 x 10-7 evs2 m2 MNacı = 6.0 × 10-7 eVs2 m2 MNa = 2.3 x 10-7 eVs2 m2 and the temperature Mclz of the system is . A useful constant is T = 300k 0.26 eV. A useful constant is h = 6.58 x 10-16eVs D) Finally, use the equilibrium constant to find how many moles of NaCl will exist in equilibrium with 1.0 mole of Na and 1.0 mole of Cl2.
Transcribed Image Text:Problem 3) Take the creation of salt from sodium and molecular chlorine: 2 Na + C12 =2 NaCl A) Write out how the equilibrium constant K will be related to the concentrations of each chemical (as variables, similar to eqn: [H2][H]-2 [H2] = K(t)). [H]2 %3D B) Write out what the equilibrium constant K will be from the quantum concentrations and internal free energy of each molecule (as variables, similar to eqn: log K = log no (H2) – 2 log no (H) - ) %3D C) Find the exact numerical equilibrium constant if the internal free energies are equal to the dissociation energies (FNa = 0, FNaci = -4.26 eV, and Fci = -2.48 e), and the masses are = 7.3 x 10-7 evs2 m2 MNacı = 6.0 × 10-7 eVs2 m2 MNa = 2.3 x 10-7 eVs2 m2 and the temperature Mclz of the system is . A useful constant is T = 300k 0.26 eV. A useful constant is h = 6.58 x 10-16eVs D) Finally, use the equilibrium constant to find how many moles of NaCl will exist in equilibrium with 1.0 mole of Na and 1.0 mole of Cl2.
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