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MakcuM [25]
3 years ago
14

What is the distance to a star whose parallex is 0.1 sec?

Physics
1 answer:
Arte-miy333 [17]3 years ago
6 0

Answer:

30.86\times 10^{13} km

Explanation:

Given the parallex of the star is 0.1 sec.

The distance is inversely related with the parallex of the star. Mathematically,

d=\frac{1}{P}

Here, d is the distance to a star which is measured in parsecs, and P is the parallex which is measured in arc seconds.

Now,

d=\frac{1}{0.1}\\d=10 parsec

And also know that,

1 parsec=3.086\times 10^{13} km

Therefore the distance of the star  is 30.86\times 10^{13} km away.

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2. Below what depth would a submarine have to submerge so that it would not be swayed by surface waves with a wavelength of 24 m
Travka [436]

<u>Answer:</u> Below 12m of depth, the submarine has to submerge so that it would not be swayed by surface waves

<u>Explanation:</u>

To avoid the surface waves, a submarine has to submerge below the wave base. It is the position below which the motion of the waves is negligible.

This wave base is equal to half of the wavelength. The equation becomes:

Wave base = \frac{\text{Wavelength}}{2}

We are given:

Wavelength = 24 m

Putting values in above equation, we get:

Wave base = \frac{24m}{2}=12m

Hence, below 12m of depth, the submarine has to submerge so that it would not be swayed by surface waves

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3 years ago
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When an object is heated, its molecules
Julli [10]

Answer:

A

Explanation:

As an object gets hotter the faster the molecules go

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4 years ago
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Nataly_w [17]

Answer: did you get the answers?

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5 0
3 years ago
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Phosphorous reacts with chlorine gas to produce phosphorous pentachloride. Calculate the mass of product produced when 25.0 g of
MariettaO [177]

Answer : The mass of product produced if the reaction occurred with a 70.5 percent yield will be, 20.67 grams.

Explanation : Given,

Mass of P = 25 g

Mass of Cl_2 = 25 g

Molar mass of P = 30.97 g/mole

Molar mass of Cl_2 = 71 g/mole

Molar mass of PCl_5 = 208.24 g/mole

First we have to calculate the moles of P and Cl_2.

\text{Moles of }P=\frac{\text{Mass of }P}{\text{Molar mass of }P}=\frac{25g}{30.97g/mole}=0.807moles

\text{Moles of }Cl_2=\frac{\text{Mass of }Cl_2}{\text{Molar mass of }Cl_2}=\frac{25g}{71g/mole}=0.352moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

2P+5Cl_2\rightarrow 2PCl_5

From the balanced reaction we conclude that

As, 5 moles of Cl_2 react with 2 moles of P

So, 0.352 moles of Cl_2 react with \frac{2}{5}\times 0.352=0.1408 moles of P

That means, in the given balanced reaction, Cl_2 is a limiting reagent and it limits the formation of products and P is an excess reagent because the given moles are more than the required moles.

Now we have to calculate the moles of PCl_5.

As, 5 moles of Cl_2 react with 2 moles of PCl_5

So, 0.352 moles of Cl_2 react with \frac{2}{5}\times 0.352=0.1408 moles of PCl_5

Now we have to calculate the mass of PCl_5.

\text{Mass of }PCl_5=\text{Moles of }PCl_5\times \text{Molar mass of }PCl_5

\text{Mass of }PCl_5=(0.1408mole)\times (208.24g/mole)=29.32g

Now we have to calculate the mass of product produced (actual yield).

\%\text{ yield of }PCl_5=\frac{\text{Actual yield of }PCl_5}{\text{Theoretical yield of }PCl_5}\times 100

70.5=\frac{\text{Actual yield of }PCl_5}{29.32g}\times 100

\text{Actual yield of }PCl_5=20.67g

Therefore, the mass of product produced if the reaction occurred with a 70.5 percent yield will be, 20.67 grams.

3 0
4 years ago
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