Calculate the energy of a photon of electromagnetic radiation at 503 nm (wavelen

Question

Calculate the energy of a photon of electromagnetic radiation at 503 nm (wavelength of maximum solar radiation) by filling in the following blank to enter your answer:
x 10 J
Enter your answer numerically. Be sure to use three significant figures for the digits portion of the scientific notation template.












Ionization involves completely removing an electron from an atom. Light of a particular wavelength can cause ionization to occur if it has the required energy.
The energy to ionize a certain element is 445 kJ/mol. What wavelength contains enough energy in a single photon to ionize one atom of this element?
Enter your answer numerically, in terms of nm and to three significant figures.

Calculate the energy of a photon of electromagnetic radiation at 503 nm (wavelength of maximum solar radiation) by filling in the following blank to enter your answer:
x 10 J
Enter your answer numerically. Be sure to use three significant figures for the digits portion of the scientific notation template.












Ionization involves completely removing an electron from an atom. Light of a particular wavelength can cause ionization to occur if it has the required energy.
The energy to ionize a certain element is 445 kJ/mol. What wavelength contains enough energy in a single photon to ionize one atom of this element?
Enter your answer numerically, in terms of nm and to three significant figures.

Calculate the energy of a photon of electromagnetic radiation at 503 nm (wavelength of maximum solar radiation) by filling in the following blank to enter your answer:
x 10 J
Enter your answer numerically. Be sure to use three significant figures for the digits portion of the scientific notation template.












Ionization involves completely removing an electron from an atom. Light of a particular wavelength can cause ionization to occur if it has the required energy.
The energy to ionize a certain element is 445 kJ/mol. What wavelength contains enough energy in a single photon to ionize one atom of this element?
Enter your answer numerically, in terms of nm and to three significant figures.
Ionization involves completely removing an electron from an atom. Light of a particular wavelength can cause ionization to occur if it has the required energy.
The energy to ionize a certain element is 445 kJ/mol. What wavelength contains enough energy in a single photon to ionize one atom of this element?
Enter your answer numerically, in terms of nm and to three significant figures.

Explanation / Answer

use,
E = (h*c)/(wavelength)
h = planck constant
= (6.6*10^-34) Js
c = speed of light
= (3*10^8) m/s
wavelength = 503 nm
= (503*10^-9) m
so,
E = {(6.6*10^-34)*(3*10^8)}/(503*10^-9)
= (3.94*10^-19) J

Answer : (3.94*10^-19) J

energy to ionise certain element is 445 KJ/mol
1 mole of element required = 445 KJ
(6.02*10^23) element required = 445 KJ
1 element required = (445/(6.02*10^23)) KJ
= (7.39*10^-22) KJ
= (7.39*10^-19) J

let wavelength be x in m
use,
E = (h*c)/(wavelength)
7.39*10^-19 = {(6.6*10^-34)*(3*10^8)}/x
7.39*10^-19 = (19.8*10^-26)/x
x = (2.68*19^-7) m
= (268*19^-9) m
= 268 nm

Answer : 268 nm

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