This question has several parts that must be sequentiam the values in listed below instead of the textbook values. Derivation Calculate the equilibrium constant for the following reaction at 1224 K. 12(g) = 2 1(g) The bond length of I2 is 2.67 Å, and the vibrational wavenumber is 214.5 cm-1. The bond dissociation energy of I₂ is 151.0 kJ-mol-1. [Hint: To calculate the degeneracy of the iodine atom in its ground electronic state, note that there is an unpaired electron in the 5p orbital. The degeneracy is given by (2J + 1), where J, the total angular momentum, is given by the sum of the orbital angular momentum and spin angular momentum. (Assume a standard pressure of 1.00 bar and a mass of 126.90 amu for I.)] Step 1 of 11 Provide the equation needed to calculate the translational partition function for the iodine atom. (Use the following as necessary: h, KB, m, 7, T, and V.) (), atrans,I= (2πmk) h³ (2πmkgT) V Step 2 of 11 Substitute numerical values into the equation from Step 1 to calculate the value of the translational partition function for the iodine atom. trans,1 1.704e-3 X Submit

The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone.   (1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)Δ?∘rxn=−122.8 kJ (2)2O3(g)⟶3O2(g)Δ?∘rxn=−285.3 kJ (3)O3(g)+Cl(g)⟶ClO(g)+O2(g)   Δ?∘rxn= ?

Which are important thermodynamic parameters associated with the completion of a single step reaction? Explain its energy profile diagram. Sketch diagrams for exo-and endothermic reactions?

True or False: 1. The initial concentration of an intermediate is assumed as 0  when using steady-state approximation. 2. A spontaneous reaction with ΔG = -1070 J/mol happens at 562 K, the Keq of this process is less than 1.