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kenny6666 [7]
3 years ago
7

A barometer can track the activity of storms at different altitudes. true of false

Chemistry
2 answers:
Bogdan [553]3 years ago
8 0
Its all the way round true 99.9% sure because they launch baometers up in the air and it reflects off of the satalght

Mazyrski [523]3 years ago
7 0

The answer is false i just took the quiz on edg.


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Calculate the frequency of the n=2 line in the lyman series of hydrogen
Alona [7]

Answer:

Approximately 2.47\times 10^{15}\; \rm Hz.

Explanation:

The Lyman Series of a hydrogen atom are due to electron transitions from energy levels n \ge 2 to the ground state where n = 1. In this case, the electron responsible for the line started at n = 2 and transitioned to

A hydrogen atom contains only one electron. As a result, Bohr Model provides a good estimate of that electron's energy at different levels.

In Bohr's Model, the equation for an electron at energy level n (

\displaystyle - \frac{k\, Z^2}{n^2} (note the negative sign in front of the fraction,)

where

  • k = 2.179 \times 10^{-18}\; \rm J is a constant.
  • Z is the atomic number of that atom. Z = 1 for hydrogen.
  • n is the energy level of that electron.

The electron that produced the n = 2 line was initially at the

\begin{aligned} &E_{n = 2} \cr &= -\frac{k\, Z^2}{n^2} \cr &= -\frac{2.179 \times 10^{-18} \times 1}{2^2} \cr & \approx -5.4475\times 10^{-19}\; \rm J\end{aligned}.

The electron would then transit to energy level n = 1. Its energy would become:

\begin{aligned} &E_{n = 1} \cr &= -\frac{k\, Z^2}{n^2} \cr &= -\frac{2.179 \times 10^{-18} \times 1}{1^2} \cr & \approx -2.179 \times 10^{-18} \; \rm J\end{aligned}.

The energy change would be equal to

\begin{aligned}&\text{Initial Energy} - \text{Final Energy} \cr &= E_{n = 2} - E_{n = 1} \cr &= -5.4475 \times 10^{-19} - \left(-2.179 \times 10^{-18}\right) \cr & \approx 1.63425\times 10^{-18}\; \rm J \end{aligned}.

That would be the energy of a photon in that n = 2 spectrum line. Planck constant h relates the frequency of a photon to its energy:

E = h \cdot f, where

  • E is the energy of the photon.
  • h \approx 6.62607015\times 10^{-34}\; \rm J \cdot s is the Planck constant.
  • f is the frequency of that photon.

In this case, E \approx 1.63425 \times 10^{-18}\; \rm J. Hence,

\begin{aligned} f &= \frac{E}{h} \cr &\approx \frac{1.63425\times 10^{-18}}{6.62607015\times 10^{-34}} \cr & \approx 2.47 \times 10^{15}\; \rm s^{-1}\end{aligned}.

Note that 1 \; \rm Hz = 1 \; \rm s^{-1}.

6 0
3 years ago
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