posted by Perez on .
A two-liter plastic soft drink bottle can withstand a pressure of 5.00 atm. Half a cup (approximately 120mL) of ethyl alcohol, (d=0.789g/mL) is poured into a soft drink bottle at room temperature. The bottle is then heated to 100C (3sig figs), changing the liquid alcohol to a gas. What is the pressure caused by the gas?
Pf= 4.65(.120)/297 x 373/.120 = 5.84
Can some one let me know if this is correct
PV = nRT
n = number of moles
Find the mass of ethyl alcohol = Density x Volume in mLs
Divide the mass by 1 mole C2H5OH --> n
R = 0.0821 L.atm/K.mol
T = 273 + 100 = 373K
L = 2.00 L
Substitute and solve for P
1 mole of C2H5OH = 12.011•2 + 1.00794•6 + 16.00 = 46.07 grams
First of all, density is mol./L. Therefore L x D will give you n. Then you plug in the numbers into P=nRT/V