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cupoosta [38]
3 years ago
12

A 3.00-g bullet has a muzzle velocity of 230 m/s when fired by a rifle with a weight of 25.0 N. (a) Determine the recoil speed o

f the rifle. 0.27 Correct: Your answer is correct. m/s (b) If a marksman with a weight of 650 N holds the rifle firmly against his shoulder, determine the recoil speed of the shooter and rifle. Incorrect: Your answer is incorrect.
Physics
1 answer:
goblinko [34]3 years ago
7 0

Answer:

0.27 m/s and 0.01 m/s

Explanation:

Given that

Mass of the bullet, m = 3 g = 0.003 kg

Velocity of the bullet, v = 230 m/s

Weight of the rifle, w = 25 N

From this, we know that the mass of the rifle, M = 25/9.8 = 2.55 kg

Using the law of conservation of momentum, we know that

Momentum of the gun = momentum of the bullet

M.g * V.g = m.b * v.b

2.55 * V.g = 0.003 * 230

2.55V.g = 0.69

V.g = 0.69 / 2.55

V.g = 0.27 m/s

If weight of the shooter = 650, then his mass = 650/9.8 = 66.33 kg

The recoil speed of the shooter is

0.69 / 66.33 = 0.010 m/s

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Answer:

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I hope this helps

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We wrap a light, nonstretching cable around a 10.0 kg kg solid cylinder with diameter of 38.0 cm cm . The cylinder rotates with
amm1812

Answer: 14.16

Explanation:

Given

d = 38cm

r = d/2 = 38/2 = 19cm = 0.19m

K.E = 510J

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I = 1/2*10*0.19²

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510J = 1/2Iω²

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Velocity is the block, v = ωr

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V = 14.30m/s

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The motive force would be

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6 0
3 years ago
4. The atmosphere is composed of about 78% nitrogen, 21% oxygen, and 1% argon. Typical atmospheric pressure in Boulder, Colorado
photoshop1234 [79]

<u>ANS</u>

<u>Step</u> <u>1</u> :Explanation of required formula.

According to Dalton's Law of Partial Pressures, the partial pressure of a component of a gaseous mixture depends on the mole ratio of said component and the total pressure of the gaseous mixture

i.e Pi=Xi × Ptotal,

Here we don't know exactly how many moles of the mixture we have,

but we know that 78.0% of all the molecules present in the mixture are nitrogen molecules, 21.0% are oxygen molecules, and 1% are molecules of Ar gas.

As we know, a mole is simply a very large collection of molecules. In order to have one mole of a substance, we need to have 6.022 × 1023 molecules of that substance.

This means that the actual number of moles is not important here, because the ratio that exists between the number of molecules is equivalent to the ratio that exists between the number of moles.

Hence,

<u>Step</u> <u>2</u> : Calculate of mole fraction of the mixture.

mole fraction of nitrogen = 78 /100 = 0.78

mole fraction of O2 =

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mole fraction of Argon =

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<u>Step</u> <u>3</u> : Calculate the pressure contributed by each of the mixture.

The pressure contributed by N2 = mole fraction of N2 × Total pressure = 0.78 × 0.83 atm = 0.6474 atm

The pressure contributed by O2 = 0.21 × 0.83 atm = 0.1743 atm

The pressure contributed by N2 = 0.01 × 0.83 atm = 0.0083 atm.

<u>Tha</u><u>nk</u> <u>You</u> !!!!!!

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