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Solved: A 368-g sample of water absorbs infrared radiation
Chapter 7, Problem 108P(choose chapter or problem)
Photodissociation of water
\(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+h v \rightarrow \mathrm{H}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(g)\)
has been suggested as a source of hydrogen. The \(\Delta H_{r x n}^{\circ}\) for the reaction, calculated from thermochemical data, is 285.8 kJ per mole of water decomposed. Calculate the maximum wavelength (in nm) that would provide the necessary energy. In principle, is it feasible to use sunlight as a source of energy for this process?
Questions & Answers
QUESTION:
Photodissociation of water
\(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+h v \rightarrow \mathrm{H}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(g)\)
has been suggested as a source of hydrogen. The \(\Delta H_{r x n}^{\circ}\) for the reaction, calculated from thermochemical data, is 285.8 kJ per mole of water decomposed. Calculate the maximum wavelength (in nm) that would provide the necessary energy. In principle, is it feasible to use sunlight as a source of energy for this process?
ANSWER:Step 1 of 3
From the given,
