- #1
QueenFisher
as promised:
a cylinder of volume 2x10^-3 m^3 contains a gas at a pressure of 1.50MNm^-2 and at a temperature of 300K.
calculate number of moles. i think I'm ok with this bit:
n=(pV)/(RT)
=(1.5x10^6)x(2x10^-3) all divided by 8.31x300
gives 1.2033694...
calculate number of molecules.
number of molecules=number of moles x avocado's constant
=1.2033694 x 6.023x10^23
=7.224283x10^23
calculate the actual mass of the gas if the molar mass is 0.032kg
actual mass = number of moles x molecular mass
=32 x 1.2033694
=38.5078
now calculate the mass of one molecule of the gas.
erk! which equation do i use? i can't use the half-m-c-squared-bar ones cos i don't know speeds or anything!
help is appreciated.
i have yet another one! watch this space.
a cylinder of volume 2x10^-3 m^3 contains a gas at a pressure of 1.50MNm^-2 and at a temperature of 300K.
calculate number of moles. i think I'm ok with this bit:
n=(pV)/(RT)
=(1.5x10^6)x(2x10^-3) all divided by 8.31x300
gives 1.2033694...
calculate number of molecules.
number of molecules=number of moles x avocado's constant
=1.2033694 x 6.023x10^23
=7.224283x10^23
calculate the actual mass of the gas if the molar mass is 0.032kg
actual mass = number of moles x molecular mass
=32 x 1.2033694
=38.5078
now calculate the mass of one molecule of the gas.
erk! which equation do i use? i can't use the half-m-c-squared-bar ones cos i don't know speeds or anything!
help is appreciated.
i have yet another one! watch this space.