Calculate the energy separations in joules, kilojoules per mole, and reciprocal centimeters between the levels (a) n = 2 and n = 1, (b) n = 6 and n = 5 of an electron in a box of length 2.0 nm
Calculate the energy separations in joules, kilojoules per mole, and reciprocal centimeters between the levels (a)...
6. Calculate the energy separation in joules and reciprocal centimeters between levels (a) n 2 and n-1 and (b) n = 6 and n 5 of an electron in a box of length 1 nm. What can you conclude about the energy separation as a function of quantum number for particle in a box model. Does this make sense, explain?
Calculate the energy in joules per photon and kilojoules per mol for the following. energy of one photon of red light with wavelength 666.1 nm __________________J/photon energy of one mole photons of red light with wavelength 666.1 nm __________________kJ/mol photon energy of one photon of infrared radiation whose wavelength is 1256 nm __________________J/photon energy of one photon of infrared radiation whose wavelength is 1256 nm __________________kJ/mol photon energy of one photon of ultraviolet light with a frequency of 4645000000000000 Hz...
Calculate the energy of photons, in joules per photon and kilojoules per mole, for 1000-kilocycle broadcast-band radio waves. (one kilocycle is a frequency of a thousand hertz). What is the wavelength of such photons? How does the energy compare with that for a carbon-carbon single bond?
a.) In your energy level sketch, make a vertical arrow between the levels that illustrates an electron transition from n = 5 to n = 2. Find the energy change, in joules, for a single hydrogen electron undergoing this transition. Convert the energy change to units of kilojoules per mole of electrons. Find the energy, frequency, and wavelength of the photon emitted from a single hydrogen atom whose electron undergoes the relaxation. Label each result clearly.
Calculate the wavelength (nm) and energy (kJ/mole) for an electron, in a Hydrogen atom, undergoing a transition from n = 200 to n = = 1. Type your answer in the space provided below: Enter the wavelength in nanometers and the Energy in kilojoules per mole. Wavelength (in nanometers) Energy (in kilojoules per mole) =
11. Calculate the energy of the first 3 energy levels in the hydrogen atom in Joules, dium kJ/mol. En = -2.18 x 10-18 ) E, (k/mol) 12. Calculate the wavelength of light, (in nm), needed to promote an electron in the ground state of the H atom to the 2 state 13. Calculate the wavelength of light, (in nm), needed to promote an electron in the ground state of the Hatom to the n=3 state
Use Coulomb's law to calculate the ionization energy in kilojoules per mole of an atom composed of a proton and an electron separated by 201.00 pm .
What is the change in energy, ΔE, in kilojoules per mole of hydrogen atoms for an electron transition from n=4 to n=2? Express your answer in kilojoules per mole to three significant figures.
Calculate the energy change (in kilojoules per mole) for the formation of the following substances from their elements. CaF2 (The sublimation energy for Ca is +178.2 kJ/mol, Ei1 = +589.8 kJ/mol, Ei2 = +1145kJ/mol, and the lattice energy of CaF2 is 2630 kJ/mol.) Express the energy change in kilojoules per mole to four significant digits.
and a Calculate the activation energy, E. in kilojoules per mole for a reaction at 51.0 °C that has a rate constant of 0.224 frequency factor of 7.07 x 10's-1