Which of the following is the reason that a more concentrated dye solution absorbs more light than a les concentrated solution? There are more molecules of dye in solution that can absorb photons, meaning fewer photons reach the detector, increasing absorbance. There are fewer molecules of dye in solution that can absorb photons, meaning more photons reach the detector, increasing absorbance. There are more molecules of dye in solution that can absorb isotopes. There are fewer molecules of dye in solution that can absorb electrons, meaning more electrons reach the detector, increasing absorbance. O There are more molecules of dye in solution that can absorb electrons.

A laser pulse at 500. nm contains 4.95 mJ of energy. How many photons are in the laser pulse? 1.25 x 1016 8.04 x 10-17 3.98 x 10-19 1.25 x 1019

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What is the wavelength of a photon that has an energy of 7.47 x 10-19 J? 725 nm 266 nm 678 nm 325 nm 459 nm

Which of the following statements are true?     Dye molecules do not absorb visible light     Dye molecules reflect all colors of light equally     Dye molecules absorb the color complementary to the one they visibly appear to be; that is to say, blue dye absorbs orange light     Dye molecules absorb the same color as the one they visibly appear to be; that is to say, blue dye absorbs blue light     Dye molecules absorb all colors of light equally

Place the following types of electromagnetic radiation in order of increasing wavelength. ultraviolet radiation, gamma ray, radio waves radio wave < gamma ray< ultraviolet radiation gamma ray< ultraviolet radiation < radio wave gamma ray < radio wave < ultraviolet radiation radio wave < ultraviolet raidation < ma ray ultraviolet radiation < gamma ray < radio wave

What is the frequency in Hz, of a photon with an energy of 3.7 x 10-18J?   Group of answer choices 5.6 x 1015 2.5 x 10-51 1.8 x 10-16 5.4 x 10-8

Over a period of 3.0 hours, a detector sensitive to 450 nm photons collects a total of 2.3 x10 -2 J of energy. How many photons struck the detector during this period of time?

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Part A1: Do you notice any pattern in the color of the light used to detect absorbance (preset) and the color of the solution? If so, describe the pattern. What happened to the transmittance when the wavelength being detected was changed to approximately the same color as the solution? Try to come up with an explanation for this. How does the percent transmittance of the preset wavelength compare to the percent transmittance when looking at the transmittance over the entire visible spectrum? What happened to the transmittance when the width of the sample was changed? Explain why this makes sense. Explain why there was an upper maximum on the concentrations for each solution. What would happen to the absorbance or percent transmittance of a sample above that concentration? If you needed to measure the exact concentration of a solution whose concentration is above that limit, is there anything you can do?