Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

The water molecule has an \(l\) = 1 rotational level 1.01 \(\times\) 10\(^-$$^5\) eV above the \(l\) = 0 ground level. Calculate the wavelength and frequency of the photon absorbed by water when it undergoes a rotational-level transition from \(l\) = 0 to \(l\) = 1. The magnetron oscillator in a microwave oven generates microwaves with a frequency of 2450 MHz. Does this make sense, in view of the frequency you calculated in this problem? Explain.

Short Answer

Expert verified
The photon frequency is approximately 24.4 GHz and exceeds the microwave's 2.45 GHz by a factor of 10, indicating a higher frequency.

Step by step solution

01

Calculate the Energy Difference

The energy difference between the two rotational levels is given as the energy of the rotatational level when \( l = 1 \), which is \( 1.01 \times 10^{-5} \) eV.
02

Convert Energy to Joules

To convert the energy from electron volts (eV) to joules (J), use the conversion factor: \( 1 \, \text{eV} = 1.602 \times 10^{-19} \, \text{J} \). Therefore, the energy difference in joules is: \[ E = 1.01 \times 10^{-5} \, \text{eV} \times 1.602 \times 10^{-19} \, \frac{\text{J}}{\text{eV}} = 1.618 \times 10^{-24} \, \text{J}.\]
03

Relate Energy to Wavelength

Use Planck's relation \( E = \frac{hc}{\lambda} \) to find the wavelength \( \lambda \), where \( h = 6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \) and \( c = 3 \times 10^8 \, \text{m/s} \). Solve for \( \lambda \): \[ \lambda = \frac{hc}{E} = \frac{6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \times 3 \times 10^8 \, \text{m/s}}{1.618 \times 10^{-24} \, \text{J}} \approx 1.23 \times 10^{-2} \, \text{m}. \]
04

Calculate Frequency of the Photon

From the wavelength \( \lambda \), the frequency \( u \) can be found using \( c = \lambda u \). Rearranging gives: \[ u = \frac{c}{\lambda} = \frac{3 \times 10^8 \, \text{m/s}}{1.23 \times 10^{-2} \, \text{m}} \approx 2.44 \times 10^{10} \, \text{Hz}. \]
05

Compare to Microwave Frequency

Convert the microwave frequency from MHz to Hz: 2450 MHz = \( 2.45 \times 10^9 \, \text{Hz} \). The photon frequency \( 2.44 \times 10^{10} \, \text{Hz} \) we calculated is about 10 times higher than the frequency of microwaves generated by the oven's magnetron.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Energy Conversion
In many scientific contexts, energy values are often given in electron volts (eV), but it can be helpful to convert these values into joules (J) for more widespread applications. An electron volt is a unit of energy that represents the kinetic energy gained by an electron when it accelerates through an electric potential difference of one volt. To convert energy from eV to joules, the conversion factor used is that 1 eV equals approximately \( 1.602 \times 10^{-19} \) J.
For example, if we have an energy difference between rotational levels of \( 1.01 \times 10^{-5} \) eV, this can be converted to joules by multiplying with the conversion factor, resulting in \( 1.618 \times 10^{-24} \) J. This conversion is crucial because it allows us to make use of joules in calculations involving Planck's constant and other fundamental constants, which are generally expressed in joules.
Understanding how to make these conversions enables the use of different scientific principles to solve problems involving energy transitions, such as those encountered in rotational spectra.
Frequency Calculation
Frequency is an important property of waves, including electromagnetic waves like light. It is defined as the number of wave cycles that pass a point per second and is measured in hertz (Hz). In order to determine the frequency of a photon absorbed during a rotational-level transition, such as from \( l = 0 \) to \( l = 1 \), we must first find the wavelength.
Using Planck's relation \( E = \frac{hc}{\lambda} \) where \( E \) is energy, \( h \) is Planck's constant \( (6.626 \times 10^{-34} \, \text{J} \cdot \text{s}) \), and \( c \) is the speed of light \( (3 \times 10^8 \, \text{m/s}) \), we can rearrange this equation to solve for frequency \( u \) once we know the wavelength \( \lambda \). We find that \( u = \frac{c}{\lambda} \).
For this particular problem, if we calculate \( \lambda \) to be approximately \( 1.23 \times 10^{-2} \, \text{m} \), the frequency \( u \) of the photon is about \( 2.44 \times 10^{10} \) Hz. Frequency calculation gives us deeper insight into the properties of light and the types of transitions it can induce.
Wavelength Determination
The wavelength of a photon involved in a transition can be determined using its relationship with energy and frequency. In the equation \( E = \frac{hc}{\lambda} \), wavelength \( \lambda \) can be isolated to find \( \lambda = \frac{hc}{E} \).
Using the constants \( h = 6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \) and \( c = 3 \times 10^8 \, \text{m/s} \), we can calculate the wavelength given an energy change of \( 1.618 \times 10^{-24} \) J. This results in a wavelength of approximately \( 1.23 \times 10^{-2} \, \text{m} \).
Wavelength determines the type of electromagnetic radiation; in this case, it falls in the microwave region of the spectrum. Knowing the wavelength helps in identifying where these transitions occur and can be essential in applications such as spectroscopy and communication technologies.
Microwave Frequency Comparison
When comparing frequencies, such as the calculated photon frequency and that of a microwave oven, we gain insight into the nature of electronic transitions. Here, we calculated the frequency of the photon absorbed by water during a rotational-level transition as approximately \( 2.44 \times 10^{10} \) Hz. In contrast, the microwave oven frequency is given as \( 2450 \) MHz, which converts to \( 2.45 \times 10^9 \) Hz.
This comparison highlights that the photon frequency is about 10 times higher than the frequency found in a typical microwave oven.
  • The microwave oven's frequency is used for heating food through microwave radiation, which causes polar molecules to rotate, generating heat.
  • Our calculated frequency corresponds to a different range of the electromagnetic spectrum, implicating different uses and mechanisms.
Understanding such distinctions is crucial in designing devices that interact with specific parts of the electromagnetic spectrum, further showing the interdisciplinary nature of physics, chemistry, and engineering.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Two atoms of cesium (Cs) can form a Cs \(_{2}\) molecule. The equilibrium distance between the nuclei in a \(\mathrm{Cs}_{2}\) molecule is \(0.447 \mathrm{nm} .\) Calculate the moment of inertia about an axis through the center of mass of the two nuclei and perpendicular to the line joining them. The mass of a cesium atom is \(2.21 \times 10^{-25} \mathrm{~kg}\).

When an OH molecule undergoes a transition from the \(n = 0\) to the \(n = 1\) vibrational level, its internal vibrational energy increases by 0.463 eV. Calculate the frequency of vibration and the force constant for the interatomic force. (The mass of an oxygen atom is \(2.66 \times 10^{-26}\) kg, and the mass of a hydrogen atom is \(1.67 \times 10^{-27} kg.)\)

Compute the Fermi energy of potassium by making the simple approximation that each atom contributes one free electron. The density of potassium is \(851 kg/m^{3}\), and the mass of a single potassium atom is \(6.49 \times 10^{-26}\) kg.

The gap between valence and conduction bands in diamond is 5.47 eV. (a) What is the maximum wavelength of a photon that can excite an electron from the top of the valence band into the conduction band? In what region of the electromagnetic spectrum does this photon lie? (b) Explain why pure diamond is transparent and colorless. (c) Most gem diamonds have a yellow color. Explain how impurities in the diamond can cause this color.

To determine the equilibrium separation of the atoms in the HCl molecule, you measure the rotational spectrum of HCl. You find that the spectrum contains these wavelengths (among others): \(60.4 \mu m\), \(69.0 \mu m\), \(80.4 \mu m\), \(96.4 \mu m\), and \(120.4 \mu m\). (a) Use your measured wavelengths to find the moment of inertia of the HCl molecule about an axis through the center of mass and perpendicular to the line joining the two nuclei. (b) The value of \(l\) changes by \(\pm 1\) in rotational transitions. What value of \(l\) for the upper level of the transition gives rise to each of these wavelengths? (c) Use your result of part (a) to calculate the equilibrium separation of the atoms in the HCl molecule. The mass of a chlorine atom is \(5.81 \times 10^{-26}\) kg, and the mass of a hydrogen atom is \(1.67 \times 10^{-27}\) kg. (d) What is the longest-wavelength line in the rotational spectrum of HCl?

See all solutions

Recommended explanations on Physics Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free