The difference in energy between allowed oscillator states in HBr molecules is 0.330 eV. What is the oscillation frequency of this molecule?
ΔE=hf
f= ΔE/h=0.33•1.6•10⁻¹⁹/6.63•10⁻³⁴ = =7.96•10¹³ Hz
To find the oscillation frequency of an HBr molecule given the energy difference between allowed oscillator states, you can use the relationship between energy and frequency.
The energy of a photon can be calculated using the formula E = hf, where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 J · s), and f is the frequency of the photon.
In order to use this formula, we need to convert the energy difference from electron volts (eV) to joules (J).
1 eV is equal to 1.602 x 10^-19 J. Therefore, the energy difference of 0.330 eV is equal to (0.330 eV) x (1.602 x 10^-19 J/eV) = 5.286 x 10^-20 J.
Now, we can rearrange the formula to solve for f:
E = hf
f = E / h
Substituting the energy difference into the equation:
f = (5.286 x 10^-20 J) / (6.626 x 10^-34 J · s)
= 7.99 x 10^13 s^-1
This is the oscillation frequency of the HBr molecule.
To find the oscillation frequency of a molecule, we can use the formula:
frequency = (1 / h) * ΔE
Where:
- frequency is the oscillation frequency (in Hz)
- h is the Planck's constant (6.626 x 10^-34 J s)
- ΔE is the difference in energy between allowed oscillator states (in joules)
First, let's convert the energy difference from eV to joules:
1 eV = 1.602 x 10^-19 J
So, ΔE = 0.330 eV * 1.602 x 10^-19 J/eV = 5.2764 x 10^-20 J
Now we can calculate the oscillation frequency:
frequency = (1 / (6.626 x 10^-34 J s)) * (5.2764 x 10^-20 J)
frequency ≈ 7.97 x 10^13 Hz
Therefore, the oscillation frequency of the HBr molecule is approximately 7.97 x 10^13 Hz.