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)

Answer 1

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

Answer 2

R = Rydberg's constant (1.0973731568539(55) x 107 m-1)

Answer 3

Typo in equation:

1/λ = RZ^2(1/n1^2 - 1/n2^2)

Z=atomic number, which is 1 for hydrogen.

Answer 4

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 5

Answer

Answer 6

En/gy in kj / mol n=5 ton=2
break H-H bond(436)kj/mol

Answer 7

Nebera

Answer 8

Student