PLEASE HELP, WITH JUST #2. I understand number 1 with answers being 2.15x10^-22 kJ and longest wavelength being 1.88x10^3 nm.
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PLEASE HELP, WITH JUST #2. I understand number 1 with answers
being 2.15x10^-22 kJ and longest...
Data Report Sheet: The Atomic Spectra of Hydrogen A. Table 1: The Energy Levels of the...
Data Report Sheet: The Atomic Spectra of Hydrogen A. Table 1: The Energy Levels of the Hydrogen Atom Quantum Number, n Energy, kJ/mol Quantum Number, Energy, E, k/mol 1 -2.18x10/1--2.18x10J 2 -2.18x10"/2--5.45x10 B. Table 2. Calculation of Wavelengths Associated with Energy Transitions 2 1 3 4 5 E, -E, AE- 1.64 x 10J AE k.J/mol , nm thc/AE)- 121.5nm AE kJ/mol nm AE kJ/mol 3 , nm AE kJ/mol nm AE kJ/mol 5 7, nm 55 Table 3: Assignment of...
Calculate the wavelengths (nm) of the lines in the Balmer Series from the values of ninitial...
Calculate the wavelengths (nm) of the lines in the Balmer Series from the values of ninitial and nfinal using equations (4) and (2) presented in your lab. Show one sample calculation for line 1 (Balmer-a) in your lab notebook, and enter the values in the table below (whole numbers only, except for column 4, use 3 sig figs). The spectral lines are grouped into series according to n'. Lines are named sequentially starting from the longest wavelength/lowest frequency of the...
4) 74 kJ are required to heat 1 cup of water fronm room temperature to boiling....
4) 74 kJ are required to heat 1 cup of water from room temperature to boiling. The wavelength of microwave radiation in a microwave oven is 2.3 x 10-3 m. How many moles of photons are required? 5) Cesium requires a minimum energy of 188 kJ/mol for an electron to be ejected. What is the wavelength of light in nm that possesses the minimum amount of energy needed to cause the electron to eject? 5.4 Balmer-Rydberg 6) Use the Balmer-Rydberg equation to calculate...
4 Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission...
4
Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of...
.019 1. When Johann Balmer found his famous series for hydrogen in wavelengths in the visible...
.019 1. When Johann Balmer found his famous series for hydrogen in wavelengths in the visible and near ultraviolet regions from series lie in that region. On the basis of the entries in Table 11.3 and me diagram, what common characteristic do the lines in the Balmer sein Print Preview ous series for hydrogen in 1886, he was limited experimentally to car ultraviolet regions from 250 nm to 700 nm, so all the lines in his entries in Table 11.3...
fill in the blanks pls LI TIe (kJ/photon) for each calibrated wavelength and then esponding energy...
fill in the blanks pls
LI TIe (kJ/photon) for each calibrated wavelength and then esponding energy (k.J/mol) per mole by using Avogadro's number. (.5d (c) Using Figurel determines the values of quantum numbers ni and for the initial and Trattatert the transitions that give rise to each line. ectr 1 . is с я Wavelength from the calibration graph (nm) Photon energy Value of n (initial state) Value of n (final state) (kJ/mol) S4L10a 419, к) п 430.00 219Kfa 2...
Name Pre-Laboratory Assignment 1. Calculate the wavelengths of the lines in the Balmer Series from the...
Name Pre-Laboratory Assignment 1. Calculate the wavelengths of the lines in the Balmer Series from the values of ninisial and ninal using equations (4) and (2). Give the wavelength and enter the values in the table below in nanometers. Show a sample calculation here, Electronic Transitions in the Spectrum of Hvdrogen Line nn1/n -1/nfWavelength, nm 2a. For hydrogen, ionization would correspond to moving the electron from n-1 to oo, Using equation (4), calculate the ionization energy of one atom of...
Ch 27 HW (Part 2) The Hydrogen Spectrum « previous 5 of 19 next » SubmitMy...
Ch 27 HW (Part 2) The Hydrogen Spectrum « previous 5 of 19 next » SubmitMy AnswersGive Up Part B What is the wavelength of the line corresponding to n=5 in the Balmer series? Express your answer in nanometers to three significant figures. SubmitMy AnswersGive Up Part C What is the smallest wavelength λmin in the Balmer's series? Express your answer in nanometers to three significant figures. Hints SubmitMy AnswersGive Up Part D What is the largest wavelength λmax in...
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the...
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the ground state. What happens to the light and to the electron? Group of answer choices a. The light is not absorbed and the final energy of the electron is -1312 kJ/mol. b.. The light is absorbed and the final energy of the electron is −328 kJ/mol. c.. The light is not absorbed and the final energy of the electron is −1050 kJ/mol. d.. The...
please answer all 5, thanks:) attributed to stray light or impurities in the discharge lube.) Data...
please answer all 5, thanks:)
attributed to stray light or impurities in the discharge lube.) Data Analysis 1. Using the scale position reading for the hydroxen snectrum and the equation generated from your calibration curve, calculate the wavelengths (in A) for each of the four lines in the hydrogen spectrum. Compare these calculated values with the reported values. Look up the four lines that are visible in the atomic spectrum of hydrogen (Be sure to provide a reference or URL)....
Data Report Sheet: The Atomic Spectra of Hydrogen A. Table 1: The Energy Levels of the Hydrogen Atom Quantum Number, n Energy, kJ/mol Quantum Number, Energy, E, k/mol 1 -2.18x10/1--2.18x10J 2 -2.18x10"/2--5.45x10 B. Table 2. Calculation of Wavelengths Associated with Energy Transitions 2 1 3 4 5 E, -E, AE- 1.64 x 10J AE k.J/mol , nm thc/AE)- 121.5nm AE kJ/mol nm AE kJ/mol 3 , nm AE kJ/mol nm AE kJ/mol 5 7, nm 55 Table 3: Assignment of...
Calculate the wavelengths (nm) of the lines in the Balmer Series from the values of ninitial and nfinal using equations (4) and (2) presented in your lab. Show one sample calculation for line 1 (Balmer-a) in your lab notebook, and enter the values in the table below (whole numbers only, except for column 4, use 3 sig figs). The spectral lines are grouped into series according to n'. Lines are named sequentially starting from the longest wavelength/lowest frequency of the...
4
Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of...
.019 1. When Johann Balmer found his famous series for hydrogen in wavelengths in the visible and near ultraviolet regions from series lie in that region. On the basis of the entries in Table 11.3 and me diagram, what common characteristic do the lines in the Balmer sein Print Preview ous series for hydrogen in 1886, he was limited experimentally to car ultraviolet regions from 250 nm to 700 nm, so all the lines in his entries in Table 11.3...
fill in the blanks pls
LI TIe (kJ/photon) for each calibrated wavelength and then esponding energy (k.J/mol) per mole by using Avogadro's number. (.5d (c) Using Figurel determines the values of quantum numbers ni and for the initial and Trattatert the transitions that give rise to each line. ectr 1 . is с я Wavelength from the calibration graph (nm) Photon energy Value of n (initial state) Value of n (final state) (kJ/mol) S4L10a 419, к) п 430.00 219Kfa 2...
Name Pre-Laboratory Assignment 1. Calculate the wavelengths of the lines in the Balmer Series from the values of ninisial and ninal using equations (4) and (2). Give the wavelength and enter the values in the table below in nanometers. Show a sample calculation here, Electronic Transitions in the Spectrum of Hvdrogen Line nn1/n -1/nfWavelength, nm 2a. For hydrogen, ionization would correspond to moving the electron from n-1 to oo, Using equation (4), calculate the ionization energy of one atom of...
please answer all 5, thanks:)
attributed to stray light or impurities in the discharge lube.) Data Analysis 1. Using the scale position reading for the hydroxen snectrum and the equation generated from your calibration curve, calculate the wavelengths (in A) for each of the four lines in the hydrogen spectrum. Compare these calculated values with the reported values. Look up the four lines that are visible in the atomic spectrum of hydrogen (Be sure to provide a reference or URL)....
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