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Chapter 9: Problem 1263

Pressure of an ideal gas is increased by keeping temperature constant what is the effect on kinetic energy of molecules. (A) Decrease (B) Increase (C) No change (D) Can't be determined

Short Answer

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(C) No change

Step by step solution

01

Recall the Ideal Gas Law.

The Ideal Gas Law is given by the equation \[PV = nRT\], where: - P = pressure - V = volume - n = number of moles - R = universal gas constant - T = temperature Since we know that the temperature remains constant, we can examine the effects of pressure and volume on the equation.
02

Understand the relationship between pressure and volume.

As the pressure of the gas increases, the volume of the gas will decrease if the temperature remains constant (as per the problem statement). This is because the Ideal Gas Law equation shows that \(PV = \text{constant}\), when temperature is held constant.
03

Recall the formula for the average kinetic energy of gas molecules.

The formula for the average kinetic energy \(\overline{KE}\) of gas molecules can be written as \[\overline{KE} \propto T\], where proporitional sign (\(\propto\)) indicates that the average kinetic energy of the gas molecules is directly proportional to the temperature of the gas.
04

Determine the effect of increasing pressure on the kinetic energy of gas molecules.

From Steps 1 to 3, we learned that: 1. The temperature is held constant. 2. The average kinetic energy of the gas molecules is directly proportional to the temperature of the gas. Since the temperature remains constant, the average kinetic energy of the gas molecules will also remain constant (no change). Therefore, the correct answer is: (C) No change

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Most popular questions from this chapter

The pressure is exerted by the gas on the walls of the container because (A) It sticks with the walls (B) It is accelerated towards the walls (C) It loses kinetic energy (D) On collision with the walls there is a change in momentum

When the pressure on \(1200 \mathrm{ml}\) of a gas is increased from $70 \mathrm{~cm}\( to \)120 \mathrm{~cm}$ of mercury at constant temperature, the new volume of the gas will be (A) \(400 \mathrm{ml}\) (B) \(600 \mathrm{ml}\) (C) \(700 \mathrm{ml}\) (D) \(500 \mathrm{ml}\)

To what temperature should the hydrogen at \(327^{\circ} \mathrm{C}\) cooled at constant pressure, so that the root mean square velocity of its molecules become half of its previous value (A) \(-100^{\circ} \mathrm{C}\) (B) \(123^{\circ} \mathrm{C}\) (C) \(0^{\circ} \mathrm{C}\) (D) \(-123^{\circ} \mathrm{C}\)

A cylinder contains \(10 \mathrm{~kg}\) of gas at pressure of $10^{\prime} \mathrm{N} / \mathrm{m}^{2}$. The quantity of gas taken out of the cylinder, if final pressure is \(2.5 \times 10^{6} \mathrm{Nm}^{-2}\). will be (temperature of gas is constant) (A) \(5.2 \mathrm{~kg}\) (B) \(3.7 \mathrm{~kg}\) (C) \(7.5 \mathrm{~kg}\) (D) \(1 \mathrm{~kg}\)

For a gas \(\left(R / C_{V}\right)=0.67\). This gas is made up of molecules which are (A) Diatomic (B) monoatomic (C) polyatomic (D) mixture of diatomic and polyatomic molecules
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