If the density of an unknown gas is 3.20 g/L at -18 degrees C and 1650 mm Hg, what is the mol mass of this gas?
I suggest looking at your textbook.
all that stuff is literally ONE equation. If you cannot get it figured out you will be a complete failure in the class.Defiance wrote:
I suggest looking at your textbook.
Someone (S.Lythberg ) correct me if I'm wrong:
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
all out guess, shot in the dark:
83.8 g/mol
let me remind you that is an absolute guess
83.8 g/mol
let me remind you that is an absolute guess
if you're having problems with this one then you're screwed.
Don't forget to convert mm Hg to atm; or the constant you point out is incorrect. Should be 1650 mm Hg / 760 mm Hg ~ 2.17 atmHurricaИe wrote:
Someone (S.Lythberg ) correct me if I'm wrong:
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
I can see where you be confused, since you do have to assume that there is one liter present.
shit was SO cash... good thing you pointed that outSmithereener wrote:
Don't forget to convert mm Hg to atm; or the constant you point out is incorrect. Should be 1650 mm Hg / 760 mm Hg ~ 2.17 atmHurricaИe wrote:
Someone (S.Lythberg ) correct me if I'm wrong:
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
Geek alert, everyone run!HurricaИe wrote:
Someone (S.Lythberg ) correct me if I'm wrong:
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
Emo alert, everyone grab the Zoloft!Ryan wrote:
Geek alert, everyone run!HurricaИe wrote:
Someone (S.Lythberg ) correct me if I'm wrong:
PV=nRT
Pressure times Volume = number of moles of gas times R (.0821) times temperature (in kelvin)
To find kelvin, add 273 to your temperature in celsius
Assume volume is 1 liter. Solve for N. Then use conversion factors to find out the molar mass (should be 3.20g/L times 1L/N)
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