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Chapter 19: Q22P (page 578)

Question: Find the rms speed of argon atoms at 313 K.Molar mass of argon atoms is 39.948 g/ mol.

Short Answer

Expert verified

Answer:

The RMS speed of argon atom is 442 m /s.

Step by step solution

01

Understanding the concept

We can find the RMS speed using its formula in terms of R, temperature, and molar mass.

The expression for the RMS speed is given by,

$v = \sqrt{\frac{3 R T}{M}}$

02

Calculate the rms speed of argon atoms

The RMS speed of argon atoms is,

$v = \sqrt{\frac{3 RT}{M}}$

Molar mass of argon is $M = 39.95 \times 10^{- 3} kg / mol .$

$v = \sqrt{\frac{3 (8.314) (313)}{39.95 \times 10^{- 3}}} v = 442.058 \approx 442 m / s$

Therefore the RMS speed of argon atoms is 442 m /s .

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Most popular questions from this chapter

An ideal diatomic gas, with rotation but no oscillation, undergoes an adiabatic compression. Its initial pressure and volume are $1.20 a t m$ and $0.200 m^{3}$ . Its final pressure is $2.40 a t m$ . How much work is done by the gas?

We give $70 J$ as heat to a diatomic gas, which then expands at constant pressure. The gas molecules rotate but do not oscillate. By how much does the internal energy of the gas increase?

Question: A beam of hydrogen molecules (H₂) is directed toward a wall, at an angle of55⁰with the normal to the wall. Each molecule in the beam has a speed of 1.0 km /s and a mass of $m = 3.3 \times 10^{- 24} g$ . The beam strikes the wall over an area of 2.0 cm², at the rate of 10²³ molecules per second. What is the beam’s pressure on the wall?

At what temperature do atoms of helium gas have the same rms speed as molecules of hydrogen gas at $20.0 ° C$ ?

Question: In the temperature range 310 K to 330 K, The pressure P of a certain non ideal gas is related to volume V and temperature T by $p = (24.9 \frac{J}{K}) \frac{T}{V} - (0.00662 \frac{J}{K^{2}}) \frac{T^{2}}{V}$

How much work is done by the gas if its temperature is raised from 315 Kto 325 Kwhile the pressure is held constant?

See all solutions

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