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)
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
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.
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
Student
To calculate the energy released when an electron transitions from one energy level to another in a hydrogen atom, we can use the equation for the energy of an electron in a hydrogen atom:
E = -13.6 * (Z^2/n^2) eV
where E is the energy in electron volts (eV), Z is the atomic number (1 for hydrogen), and n is the principal quantum number of the energy level.
To convert from electron volts to kilojoules per mole (kJ/mol), we need to multiply the energy in eV by the conversion factor of 96.4869 kJ/mol per eV.
Now let's calculate the energy released when an electron transitions from n=5 to n=2 in a hydrogen atom:
E_initial = -13.6 * (1^2/5^2) eV
= -13.6 * (1/25) eV
E_final = -13.6 * (1^2/2^2) eV
= -13.6 * (1/4) eV
ΔE = E_final - E_initial
= (-13.6 * (1/4) eV) - (-13.6 * (1/25) eV)
= (-13.6/4 + 13.6/25) eV
= (-68/20 + 544/400) eV
= (-1360/400 + 544/400) eV
= -816/400 eV
To convert eV to kJ/mol, we multiply by the conversion factor:
ΔE_kJmol = (-816/400) * 96.4869 kJ/mol/eV
= -1.6532415 kJ/mol
So, the energy released when an electron transitions from n=5 to n=2 in a hydrogen atom is approximately -1.65 kJ/mol.
Since the energy released is negative, it means that energy is being released from the system. In this case, the energy released is not sufficient to break the H-H bond, as it falls short of the required 436 kJ/mol.
Nebera
En/gy in kj / mol n=5 ton=2
break H-H bond(436)kj/mol