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I am in need of help figuring out my lab. Here are attachments of my lab. I have table 1 down but I submitted a picture because it is needed for the solutions.

I am in need of help figuring out my lab. Here are attachments of my lab. I have table 1 down but I submitted a picture because it is needed for the solutions.

Chemistry
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...
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I am in need of help figuring out my lab. Here are attachments of my lab. I have table 1 down but I submitted a picture because it is needed for the solutions. 

Questions: Quantum Number, n X 15 1000 2.179×10 J atom X given Q1) Equation 4 above gives the energy per hydrogen atom. The energies will be easier to work with if we consider a mole of atoms. Fill in the equation below, converting the constant (-2.178x10-18 -18J/atom) to units of kJ per mole. Check your answer with your instructor by email before you proceed! (Hint: If the energy is -2.178x10-18 J for one atom, will the energy become bigger or smaller for a mole of atoms? More negative, or less negative?) -1312 -1317/₁ -1312/2 -1312/3 To change 40 thg 4 5 kJ per mole (5) E, n² → energy level Q2) Theoretically, an atom has an infinite number of energy levels. However, we will focus on the first ten. Using the equation you determined in Question 1 above (giving k) per mole of atoms), complete the following table. These energies correspond to the energy of an electron in a particular energy level. Energy, En (kJ/mol) 2 E÷-2.179 × 10 J nz atam -1313 -656 Table 1 -437.33 -328 -262.4 Quantum Number, n 6 7 8 6.022x10²/13/1 mol 9 10 Energy, En (kJ/mol) -218.66 atom 1312.1938 -187.4 -164 -145.77- -131.2 1 O Plot the energy values in Table 1 on the graph on the next page by drawing a horizontal line oss the y-axis corresponding to the energy value for each of the 10 levels. Write the energy l the right end of the horizontal line. The first one (n = 1) is done for you as an example. You n see that it is difficult to get all the lines in the graph-just do the best you can!
Transcribed Image Text:Questions: Quantum Number, n X 15 1000 2.179×10 J atom X given Q1) Equation 4 above gives the energy per hydrogen atom. The energies will be easier to work with if we consider a mole of atoms. Fill in the equation below, converting the constant (-2.178x10-18 -18J/atom) to units of kJ per mole. Check your answer with your instructor by email before you proceed! (Hint: If the energy is -2.178x10-18 J for one atom, will the energy become bigger or smaller for a mole of atoms? More negative, or less negative?) -1312 -1317/₁ -1312/2 -1312/3 To change 40 thg 4 5 kJ per mole (5) E, n² → energy level Q2) Theoretically, an atom has an infinite number of energy levels. However, we will focus on the first ten. Using the equation you determined in Question 1 above (giving k) per mole of atoms), complete the following table. These energies correspond to the energy of an electron in a particular energy level. Energy, En (kJ/mol) 2 E÷-2.179 × 10 J nz atam -1313 -656 Table 1 -437.33 -328 -262.4 Quantum Number, n 6 7 8 6.022x10²/13/1 mol 9 10 Energy, En (kJ/mol) -218.66 atom 1312.1938 -187.4 -164 -145.77- -131.2 1 O Plot the energy values in Table 1 on the graph on the next page by drawing a horizontal line oss the y-axis corresponding to the energy value for each of the 10 levels. Write the energy l the right end of the horizontal line. The first one (n = 1) is done for you as an example. You n see that it is difficult to get all the lines in the graph-just do the best you can!
B. Calculation of the wavelengths of the lines in the hydrogen spectrum The observed light emitted by hydrogen is due to the transitions of electrons in hydrogen atoms from higher energy levels to lower energy levels. Therefore, the energy of the photons is calculated n (lower) Ephoton = |AE| = |Efinal - Einitial| To complete the upper half of each box, use the values of E calculated in Table 1 to find the change in energy using the equation above. For example, the AE for an electron going from the second energy level to the first is -328- (-1312) = 984. Do this for all the upper halves of the boxes. The lower half of each box is explained below. To complete the lower half of each box, calculate the wavelengths associated with the energy changes that were calculated in the upper half of the box. Use the relationship: Instructions for how to fill out Table 2. which rearranges to λ = NAhc ΔΕ where N₁ = Avogadro's constant, h = Planck's constant, and c = speed of light. 4 5 · energy level Note: Unit conversions must be performed to obtain AE and λ in the desired units. Table 2 3 051 122 3 1074 J.S 1 2 E = hc 2 ΔΕ = Nhc λ(nm) 6 5 AE (kJ/mol λ (nm) Legend for Table 2 2=hc top box bottom box n (higher) 4 E₂7 E₁ 티 (-328)-(-1312) (-32-8)-(984)- 2 984 122 (5) 1 X (6) 221 = 5207X22019 Mol ши w 9 10 -34 Page 7 of के +=65626x10 J+5) (2.998 x 16 m/s Ссабини 103 J mol =)) 6.02-X101 alom me
Transcribed Image Text:B. Calculation of the wavelengths of the lines in the hydrogen spectrum The observed light emitted by hydrogen is due to the transitions of electrons in hydrogen atoms from higher energy levels to lower energy levels. Therefore, the energy of the photons is calculated n (lower) Ephoton = |AE| = |Efinal - Einitial| To complete the upper half of each box, use the values of E calculated in Table 1 to find the change in energy using the equation above. For example, the AE for an electron going from the second energy level to the first is -328- (-1312) = 984. Do this for all the upper halves of the boxes. The lower half of each box is explained below. To complete the lower half of each box, calculate the wavelengths associated with the energy changes that were calculated in the upper half of the box. Use the relationship: Instructions for how to fill out Table 2. which rearranges to λ = NAhc ΔΕ where N₁ = Avogadro's constant, h = Planck's constant, and c = speed of light. 4 5 · energy level Note: Unit conversions must be performed to obtain AE and λ in the desired units. Table 2 3 051 122 3 1074 J.S 1 2 E = hc 2 ΔΕ = Nhc λ(nm) 6 5 AE (kJ/mol λ (nm) Legend for Table 2 2=hc top box bottom box n (higher) 4 E₂7 E₁ 티 (-328)-(-1312) (-32-8)-(984)- 2 984 122 (5) 1 X (6) 221 = 5207X22019 Mol ши w 9 10 -34 Page 7 of के +=65626x10 J+5) (2.998 x 16 m/s Ссабини 103 J mol =)) 6.02-X101 alom me
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