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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

\(2 \mathrm{~g}\) of \(\mathrm{O}_{2}\) gas is taken at \(27^{\circ} \mathrm{C}\) and pressure \(76 \mathrm{~mm} \mathrm{Hg}\). Find out volume of gas (ln liter) (A) \(3.08\) (B) \(44.2\) (C) \(2.05\) (D) \(2.44\)

Calculate the temperature at which \(\mathrm{rms}\) velocity of \(\mathrm{SO}_{2}\) molecules is the same as that of \(\mathrm{O}_{2}\) molecules at \(27^{\circ} \mathrm{C}\). Molecular weights of Oxygen and \(\mathrm{SO}_{2}\) are \(32 \mathrm{~g}\) and \(64 \mathrm{~g}\) respectively (A) \(327^{\circ} \mathrm{C}\) (B) \(327 \mathrm{~K}\) (C) \(127^{\circ} \mathrm{C}\) (D) \(227^{\circ} \mathrm{C}\)

The molar specific heat at constant pressure for a monoatomic gas is (A) \((3 / 2) \mathrm{R}\) (B) \((5 / 2) \mathrm{R}\) (C) \(4 \mathrm{R}\) (D) \((7 / 2) \mathrm{R}\)

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) \(-123^{\circ} \mathrm{C}\)

1 mole of gas occupies a volume of \(100 \mathrm{~m} 1\) at \(50 \mathrm{~mm}\) pressure. What is the volume occupied by two moles of gas at $100 \mathrm{~mm}$ pressure and at same temperature (A) \(50 \mathrm{ml}\) (B) \(200 \mathrm{ml}\) (C) \(100 \mathrm{ml}\) (D) \(500 \mathrm{~m} 1\)
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