What's the rms speed of the molecules?

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Homework Help Overview

The discussion revolves around calculating the root mean square (rms) speed of molecules in an ideal gas contained in a canister. The problem involves parameters such as mass, volume, and pressure of the gas.

Discussion Character

  • Exploratory, Conceptual clarification, Mathematical reasoning

Approaches and Questions Raised

  • Participants explore the relationship between pressure, volume, and temperature using the ideal gas law. Questions arise regarding the determination of temperature and the number of moles, as well as the implications of using different formulas for rms speed.

Discussion Status

Participants are actively engaging in clarifying concepts and relationships within the problem. Some guidance has been provided regarding the use of the ideal gas law, but there remains uncertainty about the number of moles and how to proceed with the calculations.

Contextual Notes

There is a noted lack of information regarding the temperature and the number of moles, which are critical for solving the problem. Participants are discussing these constraints without reaching a consensus on how to resolve them.

cdymdcool
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1. A canister containing 150kg of an ideal gas has a volume of 8 m^3. If the gas exerts a pressure of 5*10^5 Pa, what's the rms speed of the modecules?



I can't get the temperature of the canister...
 
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You don't need it. You have PV=nRT, so T=PV/nR. Leave it as that and continue solving the problem. Eventually, you should get a "nm" in your solution. What's this equal to?
 
so nm equals the #of moles times its mass, what isn't the #of moles still unknow?
 
nm is the #of moles times the molar mass (mass per mole). What's # of moles times the mass per mole?
 
ideasrule said:
nm is the #of moles times the molar mass (mass per mole). What's # of moles times the mass per mole?

I use the formula v = square root of(3kT/m), which k stands for boltzmann's constant and m stants for the mass of molecule.
 

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