# Find V rms and MM using density

1. Feb 1, 2012

### bmartz

1. The problem statement, all variables and given/known data
At 332 K and 1.28 x 10-2 atm, the density of a gas is 1.89 x 10-5 g/cm3. (a) Find vrms for the gas molecules. (b) Find the molar mass of the gas.

2. Relevant equations
Vrms=√(3RT/M) (RMS speed)
PV=nRT (Ideal Gas Law)
D=m/V (Density)
M = m/n (Molar mass = mass/number of moles)

3. The attempt at a solution
Am I doing this wrong or is Wiley Plus wrong?

From Ideal Gas Law: V = nRT/P
Sub into Density: D = m/(nRT/P) = mP/nRT = (m/n)(P/RT)
Sub Molar mass: D = MP/RT
So M = DRT/P

Sub into RMS speed: Vrms = √(3RT/(DRT/P)) = √(3P/D)

After converting the pressure to Pa, and the density to kg/cm3, I got:
a) 4.53x105 = 453000
b) 4.04x10-3 = .0000000404

Last edited: Feb 1, 2012
2. Feb 1, 2012

### jake929

What does Wiley Plus say, does it show you are off by several orders of magnitude or the that your solution is wrong altogether? Your dimensional analysis of your solution yields velocity units. Which shows you should be on the right track, but your units are inconsistant. You converted pressure from atm to Pa(N/m^2). You converted density to kg/cm^3. To be consistent convert your density to kg/m^3. You'll get a different answer, how it compares to Wiley I don't 'know.

Last edited: Feb 1, 2012
3. Feb 1, 2012

### ehild

Hi bmartz,

Your equations for the RMS speed and molar mass are correct, but the results are wrong without the units. Check your units. What are they for the RMS speed and molar mass?

Also check if 4.04 x 10-3 is really 0.0000000404?
ehild

4. Feb 2, 2012

### bmartz

Sorry about that, units that I got:
a) m/s
b) kg

Also for b that was a typo, I meant to put in 4.04x10-8.

5. Feb 2, 2012

### jake929

Vrms=√(3RT/M)=√(J/(mole*K)*K*mole/kg)
moles cancel and Kelvin cancel giving √(J/kg)=√(kg*m2/(s2*kg))=m/s