QuestionIt takes 338. $\mathrm{kJ} / \mathrm{mol}$ to break an carbon-chlorine single bond. Calculate the maximum wavelength of light for which an carbon-chlorine single bond could be broken by absorbing a single photon.
Be sure your answer has the correct number of significant digits. $\square$ nm

Studdy Solution
Convertir la longitud de onda de metros a nanómetros (1 m = $10^9$ nm).
$$\lambda = 3.54 \times 10^{-7} \text{ m} \times 10^9 \text{ nm/m}$$
$$\lambda \approx 354 \text{ nm}$$
La longitud de onda máxima de luz capaz de romper un enlace carbono-cloro al absorber un solo fotón es aproximadamente 354 nm.