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dybincka [34]
3 years ago
11

A simple pendulum consists of a point mass, m, attached to the end of a massless string of length L. It is pulled out of its str

aight-down equilibrium position by a small angle theta and released so that it oscillates about the equilibrium position in simple harmonic motion with frequency f. What will happen to the frequency if the same pendulum oscillates in simple harmonic motion on the moon instead of on Earth?
Physics
1 answer:
muminat3 years ago
8 0

Answer:

here on the surface of moon the gravity decreases so the frequency of oscillation will also decrease

Explanation:

As we know that frequency of oscillation of the simple pendulum is given as

f = \frac{1}{2\pi}\sqrt{\frac{g}{L}}

here we know

g = acceleration due to gravity at the surface of the planet

L = length of the pendulum

Now we know that the pendulum is on the surface of earth then gravity is given as

g = 9.81 m/s^2

now when same pendulum is taken to the surface of the moon then we have

g_{moon} = \frac{g}{6}

so here on the surface of moon the gravity decreases so the frequency of oscillation will also decrease

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\Delta L=  \alpha L_0 (T_f-T_i)

= (18 x 10^-6 /°C)(0.125 m)(100° C - 200 °C)

= -0.00225 m

New length = L + ΔL
= 1.25 m + (-0.00225 m)
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How does Newton's third law of motion describe forces?
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Which of the following is true about a planet orbiting a star in uniform circular motion? A. The direction of the velocity vecto
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The retina of the eye does all of the following except __________.
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C. rollback

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8 0
3 years ago
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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