Physical Chemistry

3. A chemist is investigating the chemical reaction system by which iodine and bromine react in a closed 2.00 L container at 150.0°C to produce iodine monobromide as seen in the reaction below. 12(g) + Br₂(g) ⇒ 2 1Br (g) a) Initially she places 4.00 moles each of iodine and bromine into the 2.00 L flask and allows it to reach equilibrium. At equilibrium, she analyzes the mixture and finds it to contain 0.620 moles of bromine gas. Determine the molar concentrations of each of the reactants and products at equilibrium. Use an ICE table, as set up below. (3 marks) b) Calculate the equilibrium constant, Keq, for this reaction system. (1 mark)

5. Write in full and shorthand notation the Slater derminant for Ne.

8. The first ionization energy of the ground-state He atom is 24.6 eV. The wavelength of light associated with a transition from the ground state to a particular excited state is 58.44 nm. Determine the ionization energy of the He atom in this excited state.

1-Try to balance the following stoichiometric problem: (2.5 points) K₂MnFe (solid) + SbFs (liquid) = KSbFe (liquid) + MnF3 (solid) + F2 (gas) Please write the reaction rate for each molecule. (1 point) John run this same reaction in his laboratory (open system). Supposing that the AGO of the reaction is close to -5.5 kJ/mol and the kinetics of the reaction is fast, compute the ratio between products and reagents. Explain your reasoning. (3 points)

3 - Draw the peptide WEHATEASSIGNMENTS and provide the percentage of hydrophobic and hydrophilic residues. (1.5 points) Please mutate enough residues in order to have total charge equal to 0. (1 point) Supposing that the peptide folds into an a-helix, how many H-bonds would it be able to form? (1 point)

Homework #2 - Errors in Chemical Formulas A. Find the error in the following formulas or names. Correct each example. 1. Al₂O₂ 2. (NH4)₂Cl₂ 3. K(CIO₂) 4. (OH), AI 5. Ca.(CN) 6. Pb₂NO₁ 7. NINO ₂2 8. Mg₂F 9. CIK 10. Ca₂O₂ B. Write the formulas for the following. a. Ba and Cl b. Sodium and nitrogen. c. Ca and Oxygen d. Aluminum and Carbonate, e. Ca and SO f. Iron (III) and oxygen C. Write the formula of the ionic compound formed from each of the following using the "Criss Cross" Method. a. Al and SO₂ b. Ba and CO c. Co(III) and Cl d. Fe(II) and PO e. Pb(IV) and O f. NH4 and Sulfur

2. Yttrium barium copper oxide (YBCO) is a ceramic material that displays high-temperature superconductivity. The chemical formula of YBCO is YBa₂Cu₂O+. a. What is the molar mass of YBCO? b. What is the mole fraction (also called atomic fraction) of each element in YBCO? [3] [3] c. What is the mass percent of each element in YBCO? [3]

Homework # 5 - Shapes Electron Dot Structure Draw the electron dot structures for each of the following compounds or ions using the general lewis dot structures given on the previous page. Name the shape of each. Tell if it is polar or non-polar.

Homework #6: Naming and Writing lonic Compounds A. Write the formula for the compound. 1. Calcium and lodine 2. Silver I and Bromine_ 3. Copper II Hydroxide 4. Silver I Acetate 5. Sodium and Sulfur 6. Potassium phosphorus 7. Chromium II Sulfate 8. Lithium Phosphate 9. Zinc II Nitrite 10. Manganese II lodine B. Identify the following as properties of ionic compounds, covalent compounds, or metallic bonds.

1. This question is about zirconium (Zr). a. How many protons, neutrons, and electrons are in *Zr and *Zr++? b. Write the ground state electron configuration of 92Zr and 9²Zr++ c. In your own words, define the term isoelectronic. d. Give one example of an atom or element that is isoelectronic with $2Zr** e. Using ⁹2Zr and $5Zr as an example, explain in your own words what an isotope is.