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alexira [117]
2 years ago
7

In fireworks, the heat of the reaction of an oxidizing agent, such as KClO₄, with an organic compound excites certain salts, whi

ch emit specific colors. Strontium salts have an intense emission at 641 nm, and barium salts have one at 493 nm.
(a) What colors do these emissions produce?
Chemistry
1 answer:
Flauer [41]2 years ago
4 0
  • In the visible spectrum, strontium exhibits a red hue at a wavelength of 641 nm in its salts.
  • In the visible spectrum, barium salts emit a green color at a wavelength of 493 nm.
<h3>What is oxidizing agent?  </h3>
  • An oxidizing agent is a substance that obtains or "accepts" or "receives" an electron from a reducing agent in a redox chemical process.
  • Or to put it another way, an oxidizer is anything that oxidizes something else.
  • Halogens, potassium nitrate, and nitric acid are a few examples of oxidizing substances.
  • A reducing agent, also known as a reductant, gets oxidized and loses electrons during a chemical process.
  • The electron donor, or reducing agent, is a substance that is normally in one of its lower potential oxidation states.

Learn more about oxidizing agent here:

brainly.com/question/11952578

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3 years ago
a water sample is found to have a cl- content of 100ppm as nacl what is the concentration of chloride in moles per liter
ladessa [460]

Answer:

The concentration of chloride ion is 2.82\times10^{-3}\;mol/L

Explanation:

We know that 1 ppm is equal to 1 mg/L.

So, the Cl^- content 100 ppm suggests the presence of 100 mg of Cl^- in 1 L of solution.

The molar mass of Cl^- is equal to the molar mass of Cl atom as the mass of the excess electron in Cl^- is negligible as compared to the mass of Cl atom.

So, the molar mass of Cl^- is 35.453 g/mol.

Number of moles = (Mass)/(Molar mass)

Hence, the number of moles (N) of Cl^- present in 100 mg (0.100 g) of Cl^- is calculated as shown below:

N=\frac{0.100\;g}{35.453\;g/mol}=2.82\times 10^{-3}\;mol

So, there is 2.82\times10^{-3}\;mol of Cl^- present in 1 L of solution.

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3 years ago
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