Asked by Billy
A mixture of argon and mercury vapor used
in advertising signs emits light of wavelength 610 nm.
Calculate the energy change resulting from
the emission of 1.00 mol of photons at this wavelength.
Answer in units of kJ/mol.
in advertising signs emits light of wavelength 610 nm.
Calculate the energy change resulting from
the emission of 1.00 mol of photons at this wavelength.
Answer in units of kJ/mol.
Answers
Answered by
Dr Russ
Use E=hc/lambda to calculate the energy (in J).
This is the energy of one photon. There are 6.02 x 10^23 particles per mole.
So energy changes is
E x 6.02 x 10^23 J/mole
or
E x 6.02 x 10^20 kJ/mole
This is the energy of one photon. There are 6.02 x 10^23 particles per mole.
So energy changes is
E x 6.02 x 10^23 J/mole
or
E x 6.02 x 10^20 kJ/mole
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