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I'm stuck on this ideal gas equation and as i have just started, i find it quite hard. Please help me on this...

calculate the molar mass of gas, which has a density of 2.615gdm³ at 298K and 101kNm-²

R= 8.31 Jkmol

gas molar volume= 22.4dm³ at STP

Any help will do! Thanks!

calculate the molar mass of gas, which has a density of 2.615gdm³ at 298K and 101kNm-²

R= 8.31 Jkmol

gas molar volume= 22.4dm³ at STP

Any help will do! Thanks!

calculate the molar mass of gas, which has a density of 2.615gdm³

The equation is PV=nRT

P= 101 kNm - you have to convert this into pascals, but i dont know how

V= 22.4 x 10^-3 (you have to convert it to m^3)

n= ???? I'm guessing molar mass is the moles??

R= 8.31

T= 298

Rearange the equation so its n= (PV)/ (RT) and put all the values in it. I dont understand the part on molar mass and the density which has been given. (sorry- hope i'm of some help!)

The equation is PV=nRT

P= 101 kNm - you have to convert this into pascals, but i dont know how

V= 22.4 x 10^-3 (you have to convert it to m^3)

n= ???? I'm guessing molar mass is the moles??

R= 8.31

T= 298

Rearange the equation so its n= (PV)/ (RT) and put all the values in it. I dont understand the part on molar mass and the density which has been given. (sorry- hope i'm of some help!)

darth_vader05

calculate the molar mass of gas, which has a density of 2.615gdm³

The equation is PV=nRT

P= 101 kNm - you have to convert this into pascals, but i dont know how

V= 22.4 x 10^-3 (you have to convert it to m^3)

n= ???? I'm guessing molar mass is the moles??

R= 8.31

T= 298

Rearange the equation so its n= (PV)/ (RT) and put all the values in it. I dont understand the part on molar mass and the density which has been given. (sorry- hope i'm of some help!)

The equation is PV=nRT

P= 101 kNm - you have to convert this into pascals, but i dont know how

V= 22.4 x 10^-3 (you have to convert it to m^3)

n= ???? I'm guessing molar mass is the moles??

R= 8.31

T= 298

Rearange the equation so its n= (PV)/ (RT) and put all the values in it. I dont understand the part on molar mass and the density which has been given. (sorry- hope i'm of some help!)

thanks for that but I still have no idea how to convert kNm-² to Pa. Do you have to covert it to atmospheres and then to Pa? But how do you do that? Also how to you convert gdm³ to m³ and getting rid of the g? I'm really confused!

I'm sorry but thats were I got stuck aswell. I had a question like that today but waited for my teacher to convert everything for me

Hopefully someone else will be able to help you!

Hopefully someone else will be able to help you!

Just a thought although not needed for this question...

PV = nRT

P can be measured in atmospheres in which case you just use the appropriate value for R (0.062)

P can be measured in KPa (KNm^-2)

to get the correct units for R just substitute a set of values at STP

V =22.41dm3

T= 273

n=1

P = (you choose)

R = this is what the sum comes to

for example

when P is in kPa

P = 101 kPa

101.3 x 22.4 = 1 x R x 273

therefore R = 8.314

When P is in atmospheres

1 x 22.4 = 1 x R x 273

R = 0.082

any of these can be used providing that you are consistent.

---------------------------------------------------------------

So on to the problem :

density of 2.615gdm³ at 298K and 101kNm-²

we have atmospheric pressure here so that for one mole of any gas occupying 22.4dm3 at STP (V1, T1)

V1/T1 = V2/T2

V2 = V1T2/T1

V2 = 22.4 x 298/273

V2 = 24.45

so one mole of this gas would occupy 22.45 litres at 298K

as the density = 2.615gdm³

then the molar mass of the gas = 22.45 x 2.615 =63.9g (it's probably SO2)

PV = nRT

P can be measured in atmospheres in which case you just use the appropriate value for R (0.062)

P can be measured in KPa (KNm^-2)

to get the correct units for R just substitute a set of values at STP

V =22.41dm3

T= 273

n=1

P = (you choose)

R = this is what the sum comes to

for example

when P is in kPa

P = 101 kPa

101.3 x 22.4 = 1 x R x 273

therefore R = 8.314

When P is in atmospheres

1 x 22.4 = 1 x R x 273

R = 0.082

any of these can be used providing that you are consistent.

---------------------------------------------------------------

So on to the problem :

density of 2.615gdm³ at 298K and 101kNm-²

we have atmospheric pressure here so that for one mole of any gas occupying 22.4dm3 at STP (V1, T1)

V1/T1 = V2/T2

V2 = V1T2/T1

V2 = 22.4 x 298/273

V2 = 24.45

so one mole of this gas would occupy 22.45 litres at 298K

as the density = 2.615gdm³

then the molar mass of the gas = 22.45 x 2.615 =63.9g (it's probably SO2)

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