II Review I C A molecular orbital calculation for H2 results in the molecular orbital diagram shown. The energy listed next to each orbital in the diagram corresponds to the energy of an electron in that orbital according to the calculation. Study the diagram and answer the questions that follow. Part A What is the ionization energy of H? +5.57 x 10-19 Express your answer numerically in kilojoules per mole. • View Avallable Hint(s) Energy -2.18x 10-18) -2.18x10-18) H H -2.51 x 10-18 ) H2 IEH = kJ/mol Submit Part B Based on the calculation, what is the ionization energy of H2 ? Express your answer numerically in kilojoules per mole. > View Available Hint(s) kJ/mol IEH, - Submit

II Review I C A molecular orbital calculation for H2 results in the molecular orbital diagram shown. The energy listed next to each orbital in the diagram corresponds to the energy of an electron in that orbital according to the calculation. Study the diagram and answer the questions that follow. Part A What is the ionization energy of H? +5.57 x 10-19 Express your answer numerically in kilojoules per mole. • View Avallable Hint(s) Energy -2.18x 10-18) -2.18x10-18) H H -2.51 x 10-18 ) H2 IEH = kJ/mol Submit Part B Based on the calculation, what is the ionization energy of H2 ? Express your answer numerically in kilojoules per mole. > View Available Hint(s) kJ/mol IEH, - 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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following reaction where an excess of water was used. AICI3(s) + 3H2O(1) → Al(OH)3(?) + 3HCI(g) Identify the physical state of Al(OH)3 and tell how you will separate it from the excess water. Select one: O A. A chemical method B. Electrolysis O C. Chromatography O D. Distillation O E. Filtration
Limestone is typically 50.0% (w/w) CaCO3. How many grams of CaCO3 are present in a limestone sample weighing 1.2 kg?
I need help with questions 1-11? Could you briefly explain which answer you got for each question?
5-
I need help with these questions (Not honor class) (Not grading)
1. What volume of 65% nitric acid with a density of 1391 kg / m ^3 can be produced from 1.5 tons of ammonia if the yield of the acid is 72%
46 gr sodium (Na) reacts with excess HCl aqueous solution according to the reaction: 2Na (s) + 2HCI(aq) → 2NaC1 (aq) + H2 According to this; which of the followings is wrong? (Na:23 21 - g/mol, ClI:35.5 g/mol, H:1 g/mol) O A) 2 gr H2 is produced B) 58.5 gr NaCl is formed O C) To consume all sodium, 2 moles of HCl is needed. D) Na atoms ionize in HCl aqueous solution. O E) 2 moles NaCl is formed
3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2Cr207 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2Cr2O7(s) [ Select ] N2(g) [ Select ] H20(L) + + [ Select ] | Cr2O3(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(g) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: o Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr20, ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr2O7 o Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] %(m/m) (NH4)2Cr2O7
Identify possible starting materials for the reaction. Y Y 1.03 2. DMS to
Select the correct starting material for the reaction shown below: 1) MgBr 2) H3O+ work up OH
You have a 11.5 mg sample of blood that contains various proteins. Hemoglobin is the only protein in the sample containing Fe. Hemoglobin contains 3.83% by mass of a compound called heme (C₃₄H₃₂FeN₄O₄, MW = 616.49 g/mol). You find that your 11.5 mg blood sample contains 34.9 micrograms of Fe. What is the mass percent of hemoglobin in your protein sample? -don't prematureley round
P1