Firework Color Emissions: Determining Energy of Strontium and Barium Salts

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SUMMARY

The discussion focuses on the color emissions of strontium and barium salts in fireworks, specifically their wavelengths and corresponding energies. Strontium salts emit an intense red color at 631 nm, while barium salts emit a blue-green color at 493 nm. The energy calculations for 1.0 g of each salt reveal that strontium emits approximately 119.8 J of photons when considering the number of atoms and their emitted energy. The participants emphasize the need for precise calculations and clarify the color description of strontium emissions as red rather than orange.

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  • Understanding of photon energy calculations using the equation E = hv
  • Familiarity with the concepts of wavelength and frequency in electromagnetic radiation
  • Basic knowledge of moles and molar mass calculations
  • Awareness of chemical reactions involving oxidizing agents like KCLO4
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  • Research the energy calculations for photon emissions in fireworks chemistry
  • Learn about the role of oxidizing agents in combustion reactions
  • Explore the properties and applications of strontium and barium salts in pyrotechnics
  • Investigate the relationship between wavelength, frequency, and energy in quantum mechanics
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Chemistry students, pyrotechnics enthusiasts, and professionals in fireworks manufacturing who seek to understand the science behind color emissions and energy calculations in fireworks displays.

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1.) In a typical fireworks device, the hat of the reaction between the strong oxidizing agent, such as KCLO4, and an organic compound excites certain salts, which emit specific colours. Strontium salts have an intense emission at 631 nm, and barium salts have one at 493 nm.

Part a was simple enough... Simply what are the colours. Strontium salts are essentially orange, and barium blue-green. Part b is as follows:

What is the energy of these emissions for 1.0g each of the chloride salts of Sr and Ba? Assume that all heat released is converted to light emitted.

I've been scanning through my lecture notes looking for an applicable equation, but E=mc^2 is reserved for nuclear reactions or relativistic rest energy, and I doubt that's what I'm looking for here... But I somewhat doubt doing a heat of formation thing would work here either. Any pointers?
 
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VenomHowell15 said:
1.) In a typical fireworks device, the hat of the reaction between the strong oxidizing agent, such as KCLO4, and an organic compound excites certain salts, which emit specific colours. Strontium salts have an intense emission at 631 nm, and barium salts have one at 493 nm.

Part a was simple enough... Simply what are the colours. Strontium salts are essentially orange, and barium blue-green. Part b is as follows:

What is the energy of these emissions for 1.0g each of the chloride salts of Sr and Ba? Assume that all heat released is converted to light emitted.

I've been scanning through my lecture notes looking for an applicable equation, but E=mc^2 is reserved for nuclear reactions or relativistic rest energy, and I doubt that's what I'm looking for here... But I somewhat doubt doing a heat of formation thing would work here either. Any pointers?

1.0 g of Sr(Cl)2 = 1/(87.6+70.9) = 6.3*10^(-3) mol of Sr

1.0 g of Ba(Cl)2 = 1/(137.3+70.9) = 4.8*10^(-3) mol of Ba

631 nm --> v = frequency = 3*10^8/6.31*10^(-7) = 4.8*10^14 Hz

493 nm --> v = 3*10^8/4.93*10^(-7) = 6.1*10^14 Hz

One photon emitted: E = hv

If every atom emits exactly one photon (I assume the question was meant in this way, but I would control this), then 6.3*10^(-3) mol of Sr atoms = [6.3*10^(-3)]*[6.0*10^23] = 3.78*10^21 Sr atoms would emit:

[3.78*10^21]*hv = [3.78*10^21]*6.6*10^(-34)*4.8*10^14

= 119.8 J of photons

You can do the same with Ba.

Make me know if the question was meant in the way I have assumed.
P.S. I would call the Sr emission "red" not "orange".
 
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