You will need to use Rydberg's equation to solve for λ. Second use λ to obtain energy of the photon.
1/λ = RZ^2(1/n1^22 - 1/n2^2)
Where n2 > n1
Solve for λ
Next solve for the energy of a photon:
E=hf
Remember,
C=λf
f=C/λ
E=h(C/λ)
C=speed of light
F=frequency
H=plank's constant
How much energy, in kilojoules per mole, is released when an electron makes a transition from n=5 to n=2 in an hydrogen atom? Is this energy sufficient to break the H-H bond (436 kj/mol is needed to break this bond)
8 answers
R = Rydberg's constant (1.0973731568539(55) x 107 m-1)
Typo in equation:
1/λ = RZ^2(1/n1^2 - 1/n2^2)
Z=atomic number, which is 1 for hydrogen.
1/λ = RZ^2(1/n1^2 - 1/n2^2)
Z=atomic number, which is 1 for hydrogen.
howmuch energy in kilojoule permole is released when an electrons makes a transition from n=5 to n=2 in an hydrogen atom? is this energy sufficient to break the H-Hbond(436kj/mole is needed to break this bond)? by symbole
Answer
En/gy in kj / mol n=5 ton=2
break H-H bond(436)kj/mol
break H-H bond(436)kj/mol
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