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bezimeni [28]
3 years ago
10

1. Two blocks travel along a level frictionless surface. Block A is initially moving to the right at 5.0 m/s, while block B is i

nitially at rest. After the collision, block A continues to the right at 1.0 m/s. The mass of block A is 2.0 kg and the mass of block B is 3.0 kg. The positive x-direction is to the right. a. Find the final velocity of block B. Show your work. b. Is the sign of the change in momentum of block A as a result of the collision positive, negative, or is it zero
Physics
1 answer:
ad-work [718]3 years ago
6 0

Answer: 2.67 m/s

Explanation:

Given

Mass of block A  is m_a=2\ kg

mass of block B is m_b=3\ kg

The initial velocity of block A u_a=5\ m/s

the initial velocity of block B is u_b=0

After collision velocity of block A is v_a=1\ m/s

Conserving momentum

m_au_a+m_bu_b=m_av_a+m_bv_b\\\\2\times 5+3\times0=2\times 1+3\times v_b\\\\v_b=\dfrac{8}{3}=2.67\ m/s

The momentum of block A after the collision is P_a=2\times 1=2\ kg.m/s

Therefore, there is no change in sign.

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A container with volume 1.64 L is initially evacuated. Then it is filled with 0.226 g of N2N
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Answer:

0.015 atm

Explanation:

The pressure of the gas can be calculated using Ideal Gas Law:

p = \frac{nRT}{V}

<u>Where:</u>

n: is the number of moles of the gas

R: is the gas constant = 0.082 L*atm/(K*mol)

V: is the volume of the container = 1.64 L

T: is the temperature

We need to find the number of moles and the temperature. The number of moles is:

n = \frac{m}{M}

<u>Where:</u>

M: is the molar mass of the N₂ = 14.007 g/mol*2 = 28.014 g/mol

m: is the mass of the gas = 0.226 g

n = \frac{0.226 g}{28.014 g/mol} = 8.07 \cdot 10^{-3} moles

Now, the temperature can be found using the following equation:

v_{rms} = \sqrt{\frac{3RT}{M}}    

<u>Where:</u>

R: is the gas constant = 0.082 L*atm/K*mol = 8.314 J/K*mol

v_{rms}: is the root-mean-square speed of the gas = 182 m/s

By solving the above equation for T, we have:

T = \frac{v_{rms}^{2}*M}{3R} = \frac{(182 m/s)^{2}*28.014 \cdot 10^{-3} Kg/mol}{3*8.314 J K^{-1}mol^{-1}} = 37.20 K        

Finally, we can find the pressure of the gas:

p = \frac{nRT}{V} = \frac{8.07 \cdot 10^{-3} mol*0.082 L*atm* K^{-1}*mol^{-1}*37.20 K}{1.64 L} = 0.015 atm

Therefore, the pressure of the gas is 0.015 atm.

I hope it helps you!

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Answer:

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The correct answer should be A
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