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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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Answer:

The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.

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The energy of nth energy levels of the H atom is given as:

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E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J

E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J=-4.4490\times 10^{-20} J

Energy of the seventh energy level = E_4

E_4=-2.18 \times 10^{-18} \times \frac{1}{4^2} J

E_4=-2.18 \times 10^{-18} \times \frac{1}{16} J=-1.3625\times 10^{-19} J

Energy of the light emitted will be equal to the energy difference of the both levels.

E=E_7-E_4=-4.4490\times 10^{-20} J-(-1.3625\times 10^{-19} J)

E=9.176\times 10^{-20} J

Wavelength corresponding to energy E can be calculated by using Planck's equation:

E=\frac{hc}{\lambda }

\lambda =\frac{hc}{E}=\frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{9.176\times 10^{-20}  J}=2.166\times 10^{-6} m=2166 nm

The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.

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