What is the energy of 1.7821 moles of photons with a frequency of 630.9 GHz?
What is the energy of 1.7821 moles of photons with a frequency of 630.9 GHz?
3.4. Compare the energy of a mole of photons of blue light (4.00 x 102 nm) with the energy of a mole of photons of microwave radiation having a frequency of 2.45 GHz (1 GHz = 109 s-1 ). Which has the greater energy? By what factor is one greater than the other?
Photons of what frequency are required to ionize fluorine, which has a first ionization energy of 1680 kJ/mol?
4 Determine the energy of a mole of photons with a frequency of 0.80 times 10^15 s^-1. Is this visible light? What would the temperature charge of 1000.0 grams of water if all the energy contained in the mole of photons was absorbed.
7. A 342 nm laser pulse contains 2.65 kJ of energy. How many moles of photons are in the laser pulse?
How much energy is associated with a mole (6.022 x 1023) of photons with a frequency of 4.30 x 1014 s-1 ( Answer in kJ to 3 sig figs)
A radar gun operates at a frequency of 10.5 GHz. A beat frequency of 2.46 GHz is then observed by the radar gun when it is used on a car heading towards the radar. a) Assume a temperature of 20 degrees Celsius, calculate the velocity of the car that is driving towards the officer. Give your answer in m/s and then convert to mph. b) Assuming a temperature of 0 degrees Celsius, find velocity in terms of m/s and then...
1) If photons have a frequency of 1.43x1015 s-1, what wavelength does this correspond to? Use units of nm. 2) A laser is emitting photons with a wavelength of 620.2 nm. What is the energy for 1 mole of these photons? For Planck's constant, use a value of 6.626x10-34 J s. Use units of kJ/mol.
A mole of photons has an energy of 149kJ. What is the wavelength of these photons? Please show steps.
Calculate the energy emitted per mole of photons (kJ/mol), by a neon sign with a frequency of 4.89 x 10" Hz. 2. A heat lamp produces 25.5 watts of power at a wavelength of 6.50 um. How many photons are emitted per second? (1 watt - 1 J/s) An electron in a hydrogen atom relaxes to the n-2 level emitting light of wavelength 410.2 nm. What is the value of n for the level where the electron originated? Hint: Use...
17 Calculate the energy associated with 3.00 moles of photons from red light with 750 nm wavelength. A. 479 kJ B. 160 kJ C. 215 kJ D. 320 kJ E. 640 kJ