Complete this table for visible light. Wavelength (nm) Frequency (s\") Energy (k

Question

Complete this table for visible light. Wavelength (nm) Frequency (s") Energy (kJmol) Color of light Given: Number Number a. 1710.5 4.2 x 1014 2.8 x 10-19 8 Red Number Given Number b. 515.6 5.819 x 101 232.5 Green Given: Number Number c. 580.6 5.2 x 1014 343 Yellow Number Number Given: d. 214.29 1.4× 1014 255.6 Violet Incorrect For part a, an energy calculated using E = hv or E = hc/A will have units of joules per photon. Yo need to convert to kilojoules per mole of photons. Remember, 1 kJ = 1000 J and 1 mol = 6.022 x 1023 photons

Explanation / Answer

Part A

Energy per photon = hx frequencey

= 6.626x10-34 J.sec x 4.2 x 1014 sec-1

energy for 1 mole in KJ = energy per photon x Avogadro number x 10-3 kJ /mol

= 6.626x10-34 J.sec x 4.2 x 1014 sec-1 x6.022x1023 x10-3 kJ/mol

= 167.58 kJ/mol

PartC

Energy per photon = hx frequencey

= 6.626x10-34 J.sec x 5.2 x 1014 sec-1

energy for 1 mole in KJ = energy per photon x Avogadro number x 10-3 kJ /mol

= 6.626x10-34 J.sec x 5.2 x 1014 sec-1 x6.022x1023 x10-3 kJ/mol

= 207.49 kJ/mol

Part D

Given E = 255.5 kJ/mol

Thus frequency = E /hxAvogadro number

= 255.6x 103 / 6.626x10-34 J.sec x6.022x1023

= 6.406 x 1014 per sec

wavelength = velocity / frequency

= 3.0x108 m/sec /  6.406 x 1014 per sec

=0.4683x10-6 m

= 468.3 x10-9 m

= 468.3 nm

color is blue

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