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A person is applying Dihydroxyacetone (DHA), where the amino acids of dead skin cells react following the Embden–Meyerhof biochemical pathway, which stains layers of skin orange-brown to create a tan.
The activation energy of this reaction is measured to be 183 J/mol.
The Molar Mass of Hydroxyacetone is 0.0741 kg/mol.
Calculate the momentum of the DHA particles in the pathway.

Respuesta :

Schnogendoodles

Answer:

1.839420926 x 10^8 m/s

Explanation:

A form of De Broglie's equation can be derived from Einstein's formula

of E = mc^2

E = mc^2

E = hf

mc^2 = hf

We know f = v / λ

so mc^2 = hv / λ

That means that E = hv / λ

h, λ, c = constants

It now becomes easy to plug in our values:

[tex](0.0741 kg/mol) * (2.998 *10^{-8} m/s) = \frac{(6.626*10^-34) * (v)}{(10^{-9}) }[/tex]

Solve for v

[tex]6.66 *10^{-17} = 6.626 *10^{-25} * v[/tex]

v = 100514804.7 mol*m/J*s

x Activation Energy = 183942092.6 m/s

This makes sense because the particles are photons and should be moving close to the speed of light.

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