7. Gases

Root Mean Square Speed

Root Mean Square Speed & the Assumptions of Kinetic Theory | A-level Physics | AQA, OCR, Edexcel

You have a sample of gas at 0 C. You wish to increase the
rms speed by a factor of 3. To what temperature should
the gas be heated?

CHEMISTRY 101 - Root mean square velocity of gas molecules

Root Mean Square Speed RMS vs Average Speed

⚗️ Root Mean Square Velocity (Question 1)

The coldest temperature recorded at ground level on Earth was -89.2 °C at the Vostok Station in Antarctica. What is the speed of a nitrogen molecule at this temperature? (LO 10.9)
(a) 933 m/s (b) 40.2 m/s
(c) 404 m/s (d) 12.8 m/s

Understanding kinetic energy & Root Mean Square Speed

The average temperature at an altitude of 20 km is 220 K. What 
is the average speed in m/s of an N2 molecule at this altitude?

A Level Physics: What is the root mean square speed?

Which has a higher average speed, H2 at 150 K or He at 
375 °C?

At what temperature does the average speed of an oxygen molecule equal that of an airplane moving at 580 mph?

A big-league fastball travels at about 45 m/s. At what temperature (°C) do helium atoms have this same average speed?

Root Mean Square Speed Example 1

Radon (Rn) is the heaviest (and only radioactive) member of
the noble gases. How much slower is the root-mean-square
speed of Rn than He at 300 K?

Calculate the average speed of a nitrogen molecule in m/s 
on a hot day in summer 1T = 37 °C2 and on a cold day in 
winter 1T = -25 °C2.

The root mean square speed of gas molecules is 283.0 m/s at a given temperature T when the recorded molar mass is 42.0 g/mol. What would be the root mean square speed for a gas with a molar mass of 152.0 g/mol?

In the calculation, the molar mass must be in units of kg/mol and the gas constant, R, needs to be in units of J/mol K.

In the calculation for diatomic nitrogen (N2), the molar mass must be in units of kg/mol and the gas constant, R, needs to be in units of J/mol K.

 In the calculation, the molar mass must have units of kg/mol. 

 The molar mass must be in units of kg/mol. 

Correct, &mu;rms would be larger at a higher temperature.

Molar mass must be in units of kg/mol and the gas constant, R, needs to be in units of J/mol K.

 Calculate the root mean square velocity of nitrogen molecules at 20.0&#x2103;. 

(b) Calculate the rms speed of CO molecules at 25 °C.

Determine which gas would have a root mean square speed of 515.59 m/s at 405 K.

Which has a higher average speed, a Ferrari at 145 mph or 
a gaseous UF6 molecule at 145 °C?

Calculate the root mean square velocity of
F2, Cl2, and Br2 at 298 K.

At what temperature (°C) will xenon atoms have the same 
average speed that Br2 molecules have at 20° C?

The temperature of a 5.00-L container of N2 gas is increased
from 20 °C to 250 °C. If the volume is held constant,
predict qualitatively how this change affects the following:
(b) the rootmean-square speed of the molecules.

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[BOOK CHEM] Clutch Version

Partial Pressure

Partial Pressure (PGas) is the pressure exerted by an individual gas within a container.

Velocity Distributions

Velocity Distributions represent probability distributions for a gas when examining their molar mass and temperature.

Mole Fraction

Mole Fraction (X) represents the mole component by total moles.&nbsp;

Mole Fraction -

The Ideal Gas Law Derivations

The&nbsp;Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables.&nbsp;

Root Mean Square Speed&nbsp;allows for the determination of the velocity of 1 type of gas molecule.

The Ideal Gas Law: Density

Under certain conditions of pressure and temperature, the Ideal Gas Law can determine the density&nbsp;of a gas.&nbsp;

Effusion

Effusion is the escaping of gas molecules or atoms through a pinhole.&nbsp;

Kinetic Energy of Gases

Kinetic Energy is the energy an object possesses due to its motion.

Gas Stoichiometry

Gas Stoichiometry involves chemical reactions that contain gases.

The Ideal Gas Law

The Ideal Gas Law formula relates the behavior of gases under varying conditions of pressure, volume, moles and temperature.

Chemistry Gas Laws: Combined Gas Law

The Combined Gas Law&nbsp;is created from “combining” Boyle’s Law, Charles’ Law, and Gay–Lussac’s Law.

Pressure Units

Pressure is the force that is exerted within a given volume of space.&nbsp;

Kinetic Molecular Theory

A gas is seen as a collection of molecules or individual atoms that are in constant motion. The Kinetic-Molecular Theory tries to use data of real gases to predict how an ideal gas would behave if they existed.&nbsp;&nbsp;

Standard Temperature and Pressure

In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure.&nbsp;

The Ideal Gas Law Applications

The Ideal Gas Law Applications establish both the direct and inverse relationships between the Ideal Gas Law variables.

Maxwell-Boltzmann Distribution

The Maxwell-Boltzmann Distribution is a probability distribution curve that describes the speed of a gas at a specific temperature.

Chemistry Gas Laws

Chemistry Gas Laws&nbsp;are laws that relate together the pressure, volume and temperature of a gas.

The Ideal Gas Law: Molar Mass

The Ideal Gas Law can be further extended to find the molar mass of a gas.&nbsp;

Van der Waals Equation

The&nbsp;Van der Waals Equation is used when dealing with real, non-ideal gases.&nbsp;