## Chemistry: Principles and Practice (3rd Edition)

$1.48\times10^{3} kJmol^{-1}$
E= hν h = $6.626\times10^{-34}Js$ ν = $3.70\times10^{15}Hz$ E = $(6.626\times10^{-34}Js)(3.70\times10^{15}s^{-1})$ = $2.45\times10^{-18}J$ Energy of one mole of photons = ($2.45\times10^{-18}J$)($6.022\times10^{23}mol^{-1}$) = $1.48\times10^{3} kJmol^{-1}$.