A gaseous compound has a density of 1.90 g/L at 51.1 ∘C and 1.09 bar . Assuming ideal behavior, calculate the molar mass of the
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There is a specific formula to use for these type of problems.
ln (P2/ P1)= Δvap/ R x (1/T1 - 1/T2)
R= 8.314
P1= 92.0 torr
T1= 23 C + 273= 296 K
P2= 351.0 torr
T2= 45.0 C + 273= 318 K
plug the values and solve for the unknown
ln( 351.0/ 92.0)= Δvap/ 8.314 x (1/296 - 1/318)
Δvap= 47630.6 joules
ln (P2/ P1)= Δvap/ R x (1/T1 - 1/T2)
R= 8.314
P1= 92.0 torr
T1= 23 C + 273= 296 K
P2= 351.0 torr
T2= 45.0 C + 273= 318 K
plug the values and solve for the unknown
ln( 351.0/ 92.0)= Δvap/ 8.314 x (1/296 - 1/318)
Δvap= 47630.6 joules