Posted by Karen on Wednesday, November 7, 2007 at 3:53pm.
That is 495 what? J/mol? kJ/mol? kJ/molecule. J/atom? just what?
Use E = hc/lambda where E is Joules, h is Planck's constant = 6.626 x 10^-34, c = speed of light in m/s (3 x 10^8 m/s)
and lambda will be in meters. To determine frequency, use c = lamda x freq.
For #2.
Use PV = nRT. I would convert kPa to atmospheres, T remember is in Kelvin, R is 0.08205 L*atm/mol*K, V must be in liters. Calculate n and from that determine how many molecules of O2 you have. The way I read the problem 1 photon is required to break 1 bond; therefore, you simply need to know how many bonds there are to be broken.
Post your work if you get stuck.
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