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3 years ago

Which best explains how the diffraction pattern observed in Young’s experiment supports the wave theory of light?

Chemistry

2 answers:

olganol [36]3 years ago

4 0

C. The pattern was caused by the interference of waves.

Damm [24]3 years ago

3 0

Answer: The correct answer is option C.

Explanation:

The experiment performed by Thomas Young was named as double-slit experiment. In this experiment, he demonstrated the wave theory of the light.

In the experiment, he took a point source of light which illuminated two narrow adjacent slits on the screen and the image formed by the light were passed through the slits and was observed on the second screen.

The regions of dark and light regions were called as interference fringes which were caused by the constructive and the destructive interference of light waves.

Hence, he concluded that the pattern that was caused was due to the interference of the waves.

Therefore, the correct answer is Option C.

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Answer

Manual samplers are prone to effects of temperature, speed of wind and air concentrations.

Explanation

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3 years ago

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3 years ago

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If an element only partially conducts electricity, it would be part of the _______ category. *

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It would be in the transition metals

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3 years ago

Chemistry help! Zoom in to see better!!

inna [77]

Answer:

11.9 g of nitrogen monoxide

Explanation:

We'll begin by calculating the number of mole in 6.75 g of NH₃. This can be obtained as follow:

Mass of NH₃ = 6.75 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 6.75 / 17

Mole of NH₃ = 0.397 mole

Next, we shall determine the number of mole of NO produced by the reaction of 0.397 mole of NH₃. This can be obtained as follow:

4NH₃ + 5O₂ —> 4NO + 6H₂O

From the balanced equation above,

4 moles of NH₃ reacted to produce 4 moles of NO.

Therefore, 0.397 mole of NH₃ will also react to produce 0.397 mole of NO.

Finally, we shall determine the mass of 0.397 mole of NO. This can be obtained as follow:

Mole of NO = 0.397 mole

Molar mass of NO = 14 + 16 = 30 g/mol

Mass of NO =?

Mass = mole × molar mass

Mass of NO = 0.397 × 30

Mass of NO = 11.9 g

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3 years ago

Suppose that Daniel has a 3.00 3.00 L bottle that contains a mixture of O 2 O2 , N 2 N2 , and CO 2 CO2 under a total pressure of

Alenkinab [10]

Answer:

Partial pressure O₂ → 2.74 atm

Explanation:

Let's analyse the data given:

Volume → 3L

In the bottle there is a mixture of gases that contains, O₂, N₂ and CO₂.

Total pressure is 4.80 atm

Let's apply the Ideal Gases Law to determine the total moles of the mixture

P . V = n . R. T

4.80 atm . 3L = n . 0.082 . 273K

n = 4.80 atm . 3L / 0.082 . 273K → 0.643 moles

We apply the concept of mole fraction:

Mole fraction of a gas X = moles of gas X / Total moles

Mole fraction of a gas X = Partial pressure X / Total pressure

In a mixture, sum of mole fraction of each gas = 1

We determine mole fraction of N₂ → 0.230 / 0.643 = 0.357

We determine mole fraction of CO₂ → 0.350 atm / 4.80 atm = 0.0729

1 - mole fraction N₂ - mole fraction CO₂ = mole fraction O₂

1 - 0.357 - 0.0729 = 0.5701 → mole fraction O₂

We replace in the formula: Mole fraction O₂ = Partial pressure O₂ / 4.80 atm

0.5701 . 4.80 atm = Partial pressure O₂ → 2.74 atm

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3 years ago

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