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AURORKA [14]
3 years ago
9

Two containers hold an ideal gas at the same temperature and pressure. Both containers hold the same type of gas, but container

B has twice the number of particles and twice the volume of container A. The average kinetic energy per molecule in container B is :
A. Twice that for container A

B. The same as that for container A

C. Half that for container A

D. Impossible to determine
Physics
1 answer:
sergeinik [125]3 years ago
7 0

Answer:

B. The same as that for container A

Explanation:

To calculate the average Kinetic Energy per molecule,

K_{avg} = 3/2 K_{B} T

Where K_{avg} is the average kinetic energy per molecule and K_{B} is the Boltzmann constant

From the above equation it is seen that K_{avg} only depends on the temperature of the gas

And since the temperatures of both gases are equal, their average kinetic energy per molecule is the same

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What will happen in the next moment for the girl on the swing?
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2 years ago
A long jumper can jump a distance of 7.4 m when he takes off at an angle of 45° with respect to the horizontal. Assuming he can
GenaCL600 [577]

Answer:

0.02 m

Explanation:

R₁ = initial distance jumped by jumper = 7.4 m

R₂ = final distance jumped by jumper = ?

θ₁ = initial angle of jump = 45°

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initial distance jumped is given as

R_{1}=\frac{v^{2}Sin2\theta _{1} }{g}

final distance jumped is given as

R_{2}=\frac{v^{2}Sin2\theta _{2} }{g}

Dividing final distance by initial distance

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