In fireworks, the heat of the reaction of an oxidizing agent, such as KCIO4, with an organic compound excites certain salts, which emit specific colors. Strontium salts have an intense emission at 641 nm. What is the energy (in kJ) of this emission for 3.16 g of the chloride salt of strontium? Assume that all the heat produced is converted to emitted light. Enter to 2 decimal places.

A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 66.6 g of water at 37.5°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/ °C•g and assume only the water absorbs the energy of the microwaves. S photons

The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.Which of the following statements are true and which are false. 1. it takes less energy to ionize the electron from n=3 than it does from the ground state.2. The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.3. the electron is farther from the nucleus on average in the n=3 state than in the ground state.4. The first excited state corresponds to n=3.5. The wavelength of light emitted when the electron drops from n=3 to n=2 is shorter than the wavelength of light emitted if the electron falls from n=3 to n=1.

A hydrogen atom absorbs a photon with a wavelength of 1094 nm and causes an electron to make a transition from an unknown n1 to a final n2 = 6.   Part A Calculate frequency of the absorbed photon in units of s-1.       Part B Calculate the energy change in the atom (ΔEatom in J) upon absorption of the photon.     Part C Calculate the value of n1

The minimum energy required to remove an electron from a certain metal is 3.7 x 10– 19 J. If the metal surface is struck by light having a wavelength of 5.00 x 102 nm, what is the kinetic energy of the electron ejected from the metal?

The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 6.30 × 10¹⁴ Hz. (h = 6.626 × 10⁻³⁴ J • s)

What is the energy (in J) of a photon with a frequency of 7.07 × 10¹⁴ s⁻¹? (h = 6.626 × 10⁻³⁴ J • s)

The electron microscope uses the wave property of electrons to observe very small objects. A moving electron has a wavelength described by the de Broglie equation. What would be the kinetic energy, in J, of an electron with a wavelength of 0.485 nm, which would be equivalent to the wavelength of electromagnetic radiation in the X-ray region? (The mass of an electron is 9.11 × 10-28 g.)

The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 6.70 × 1014 Hz. (h = 6.626 × 1034 J•s)

Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with 1.00 mol of photons with a wavelength of 320. nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to? Energy = kJ/mol