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Anna35 [415]
3 years ago
11

Which of the following statements is true about the food chain below? Grass ⇒ grasshopper ⇒ bird ⇒ hawk The amount of energy tra

nsferred from the grass to the grasshopper is ____. the amount of energy transferred from the grasshopper to the bird.
A)More than
B)Less than
C)The same as
Chemistry
2 answers:
lorasvet [3.4K]3 years ago
8 0

In a food chain we arrange the energy in the form of a pyramid.

The producers are on the base of pyramid and then consumers are towards peak.

in the given food chain grass is being eaten by grasshopper which are food of birds.

Grasshoppers are also eaten up by Hawks. so both brids and hawks are feeding upon grasshoppers thus the amount of energy transferred from the grass to the grasshopper is the same as the amount of energy transferred from the grasshopper to the bird.

Taya2010 [7]3 years ago
8 0

Answer: Option (C) is the correct answer.

Explanation:

In the given case, the amount of energy transferred from the grass to the grasshopper is more, because in each stage of the food chain, some energy is lost in the form of heat. The transfer of energy becomes more inefficient the more you climb up in the food chain.

Thus, we can conclude that the amount of energy transferred from the grass to the grasshopper is more than the amount of energy transferred from the grasshopper to the bird.

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Use the Rydberg Equation to calculate the energy in Joules of the transition between n = 7 and n = 3 for the hydrogen atom. Find
Vladimir79 [104]

Answer:

The energy of each transition is approximately 1.98\times 10^{-19}\; \rm J.

The frequency of photons released in such transitions is approximately 3.00\times 10^{14}\; \rm Hz.

Explanation:

The Rydberg Equation gives the wavelength (in vacuum) of photons released when the electron of a hydrogen atom transitions from one main energy level to a lower one.

  • Let \lambda_\text{vac} denote the wavelength of the photon released when measured in vacuum.
  • Let R_\text{H} denote the Rydberg constant for hydrogen. R_\text{H} \approx 1.09678 \times 10^{7}\; \rm m^{-1}.
  • Let n_1 and n_2 denote the principal quantum number of the initial and final main energy level of that electron. (Both n_1\! and n_2\! should be positive integers; n_1 > n_2.)

The Rydberg Equation gives the following relation:

\displaystyle \frac{1}{\lambda_\text{vac}} = R_\text{H} \cdot \left(\frac{1}{{n_2}^2}} -\frac{1}{{n_1}^2}\right).

Rearrange to obtain and expression for \lambda_\text{vac}:

\displaystyle \lambda_\text{vac} = \frac{1}{\displaystyle R_\text{H}\cdot \left(\frac{1}{{n_2}^2} - \frac{1}{{n_1}^2}\right)}.

In this question, n_1 = 7 while n_2 = 3. Therefore:

\begin{aligned} \lambda_\text{vac} &= \frac{1}{\displaystyle R_\text{H}\cdot \left(\frac{1}{{n_2}^2} - \frac{1}{{n_1}^2}\right)} \\ &\approx \frac{1}{\displaystyle 1.09678 \times 10^{7}\; \rm m^{-1} \cdot \left(\frac{1}{3^2} - \frac{1}{7^2}\right)} \approx 1.0 \times 10^{-6}\; \rm m \end{aligned}.

Note, that 1.0\times 10^{-6}\; \rm m is equivalent to 1000\; \rm nm. That is: 1.0\times 10^{-6}\; \rm m = 1000\; \rm nm.

Look up the speed of light in vacuum: c \approx 3.00\times 10^{8}\; \rm m \cdot s^{-1}. Calculate the frequency of this photon:

\begin{aligned} f &= \frac{c}{\lambda_\text{vac}} \\ &\approx \frac{3.00\times 10^{8}\; \rm m\cdot s^{-1}}{1.0\times 10^{-6}\; \rm m} \approx 3.00 \times 10^{14}\; \rm Hz\end{aligned}.

Let h represent Planck constant. The energy of a photon of wavelength f would be E = h \cdot f.

Look up the Planck constant: h \approx 6.62607 \times 10^{-34}\; \rm J \cdot s. With a frequency of 3.00\times 10^{14}\; \rm Hz (1\; \rm Hz = 1\; \rm s^{-1},) the energy of each photon released in this transition would be:

\begin{aligned}E &= h \cdot f \\ &\approx 6.62607 \times 10^{-34}\; \rm J\cdot s^{-1} \times 3.00 \times 10^{14}\; \rm s^{-1} \\ &\approx 1.98 \times 10^{-19}\; \rm J\end{aligned}.

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Explanation:

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