The minimum wavelength of light required to decompose a single ozone molecule is 320.nm.Calculate the minimum energy required to decompose 1.00 mole of ozone.(h = 6.626 $\times$ 10^-34 J.s; c = 3.00 $\times$ 10⁸ m/s; 1 nm = 10^-9 m; 1mol = 6.022 $\times$ 10²³)

Question

Quizplus · Accepted Answer

The energy required to decompose 1 mole of ozone can be calculated using the equation:
E = hc/λ
where h is Planck's constant, c is the speed of light, and λ is the wavelength of light.
Substituting the given values:
E = (6.626 x 10^-34 J s) x (3.00 x 10^8 m/s) / (320 x 10^-9 m)
E = 6.21 x 10^-19 J
To convert this to kJ/mol, we need to multiply by Avogadro's number and divide by 1000:
E = (6.21 x 10^-19 J) x (6.022 x 10^23 /mol) / 1000
E = 374 kJ/mol

Therefore, the best choice is D, 374 kJ/mol, which is the correct energy required to decompose 1.00 mole of ozone.

The Minimum Wavelength of Light Required to Decompose a Single ×\times×

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