A mole of red photons of wavelength 725. 51 × 10^4 J = 165.

A mole of red photons of wavelength 725. A mole of red photons with a wavelength of 725 nm has approximately 165. 02742 × 10^-17 J E = 2. A mole of red photons with a wavelength of 725 nm has how much energy in kilojoules (kJ)? Here’s what I have done so far: Step 1 Solution To‏‏‎ ‎calculate‏‏‎ ‎the‏‏‎ ‎energy‏‏‎ ‎of‏‏‎ ‎a‏‏‎ ‎mole‏‏‎ ‎of‏‏‎ ‎red‏‏‎ ‎photons‏‏‎ ‎wit E = 6. 626 x 10^-34 Js), c is the speed of light (3 x 10^8 m/s), and λ is the wavelength (725 nm). 51 × 10^4 J = 165. 022 × 10^23 photons E (total) = 16. 1kJ Find step-by-step Physics solutions and your answer to the following textbook question: A mole of red photons of wavelength $725\ \text {nm}$ has ________ KJ of energy. 742 × 10^-19 J × 6. 022 × 10^23 photons So, the total energy of 1 mole of photons is: E (total) = 2. 2 kJ of energy. This is calculated using the formula relating energy to wavelength and multiplying by Avogadro's number. 626×3/725 × 10^ (-34+8+9) J E = 0. . We can use the formula: E = h * c / λ where E is the energy of the photon, h is Planck's constant (6. First, we need to find the energy of a single red photon. We can measure a photon's position and momentum Photons have no mass, but each photon has an amount of energy based on its frequency (number of vibrations per second) Each photon has a wavelength. 742 × 10^-19 J Therefore, for one mole of red photons, according to Avogadro's constant: 1 mole = 6. rtcvjn bne sxklc tbyf otydt pyonsujj cvgp qiim xyvpr oxmf