Question

Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (λ=465 nm).

Part B. Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction

½Cl₂(g) + ½F₂(g) → ClF(g)

Answer 1

Cive wavelength of Blue light LA2 4650m -Energy ef_1 photooshez 6.626x10341-5 X 3x108mk 465810-9 - 4.27x10-19 * Energy of 1 mol plotone = 4.27 X10-19J x 6.023X1023 Austelle 2057x1053 تا که د so, This caccede C2 | 243 kJ) and So, this light ce and f2. bond enthalpy value of F21158 kJ). can breakb onde between BI + Celzig)+ 1 Fz1g12 cif(g) we know that __AH_EMA Bonds 1EH Bonde Broken . Formed) = { 1 243) + |1ss} } - { 193} . = (199- 193) kJ 6 kJ

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