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4 years ago

What can you infer about a telescope with a large aperture? *

Chemistry

1 answer:

Tanzania [10]4 years ago

4 0

Answer:

Its images are brighter and clearer than other telescopes.

Explanation:

<em>For a telescope with large aperture, the correct answer would be that its images are brighter and clearer than those of other telescopes.</em>

The aperture of a telescope is a measure of the diameter of the optical instrument used in the telescope. The instrument could be a lens or a mirror.

<u>The larger the aperture of an optical instrument of a telescope, the more the amount of light that gets to the telescope and thus, the brighter and clearer the image taken by the telescope would be.</u>

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A 1.25-g sample contains some of the very reactive compound Al(C6H5)3. On treating the compound with aqueous HCl, 0.951 g of C6H

Oksanka [162]

<span>83.9% First, determine the molar masses of Al(C6H5)3 and C6H6. Start by looking up the atomic weights of the involved elements. Atomic weight aluminum = 26.981539 Atomic weight carbon = 12.0107 Atomic weight hydrogen = 1.00794 Molar mass Al(C6H5)3 = 26.981539 + 18 * 12.0107 + 15 * 1.00794 = 258.293239 g/mol Molar mass C6H6 = 6 * 12.0107 + 6 * 1.00794 = 78.11184 g/mol Now determine how many moles of C6H6 was produced Moles C6H6 = 0.951 g / 78.11184 g/mol = 0.012174851 mol Looking at the balanced equation, it indicates that 1 mole of Al(C6H5)3 is required for every 3 moles of C6H6 produced. So given the number of moles of C6H6 you have, determine the number of moles of Al(C6H5)3 that was required. 0.012174851 mol / 3 = 0.004058284 mol Then multiply by the molar mass to get the number of grams that was originally present. 0.004058284 mol * 258.293239 g/mol = 1.048227218 g Finally, the weight percent is simply the mass of the reactant divided by the total mass of the sample. So 1.048227218 g / 1.25 g = 0.838581775 = 83.8581775% And of course, round to 3 significant digits, giving 83.9%</span>

8 0

3 years ago

A gas at constant volume has a pressure of 4. 50 atm at 200. K. What will be the pressure of the gas at 250. K? 3. 60 atm 4. 60

Trava [24]

5.625 atm will be the pressure of the gas at 250 K temperature of the gas at constant volume.

<h3>How we calculate the pressure of the gas?</h3>

Pressure of the gas will be calculated by using the ideal gas equation as:

PV = nRT,

From the question, it is clear that:

Moles of the gas and volume is constant here, so we calculate the pressure by rearranging the above equation as:

P/T = nR/V

And required equation will be:

P₁/T₁ = P₂/T₂, where

P₁ = pressure of gas = 4.50 atm

T₁ = temperature of gas = 200 K

P₂ = pressure of gas = to find?

T₂ = temperature of gas = 250 K

On putting all these values in the above equation, we get

P₂ = 4.50 × 250 / 200 = 5.625 atm

Hence, 5.625 atm is the pressure of the gas.

To know more about ideal gas equation, visit the below link:

brainly.com/question/1056445

5 0

3 years ago

Arrange the steps in order to describe how photons and carbon dioxide contribute to the warming of earth

adell [148]

Answer:

The steps are arranged in the following order, describing how carbon dioxide and photons impact the earth's warming.

Explanation:

The sequence is in the following order;

The sun radiated sunlight (visible) photons
Photons from the sun strike the earth and become infrared photons
Earth radiates infrared photons into the atmosphere
CO2 in the atmosphere absorb infrared photons
CO2 in the atmosphere emit infrared photons back towards earth

Carbon dioxide (CO2) molecules can absorb energy from infrared (IR) radiation. Due to vibrations caused by this absorption, the CO2 molecules later release extra energy by emitting another infrared photon.

This ability of CO2 molecules to absorb and re-emit infrared energy is what makes it an effective heat-trapping greenhouse gas.

5 0

4 years ago

Find the number of atom in 1.50g of c

Aleonysh [2.5K]

Atomic mass Carbon (C ) = 12.01 a.m.u

12.01 g ---------- 6.02x10²³ atoms
1.50 g ----------- ??

1.50 x ( 6.02x10²³ ) / 12.01 =

7.51x10²² atoms of C

hope this helps!

6 0

3 years ago

How many moles of carbon dioxide are produced when 22.8g of butane react

Juliette [100K]

Butane undergoes combustion to produce carbon dioxide and water, expressed in the following reaction <span> C4H10 (g) + O2 (g) → 4CO2 (g) + 5H2O (g) . 1 mole of butane is to 4 moles of CO2. In this case, when 22.8 grams of butane or 0.393 moles of it, 69.18 grams of carbon dioxide is produced</span>

4 0

3 years ago