Chem Gas Laws?

Question

A particular balloon can be stretched to a maximum surface area of 1257 cm^2. The balloon is filled with 3.2 L of helium gas at a pressure of 759 torr and a temperature of 292K . The balloon is then allowed to rise in the atmosphere. Assume an atmospheric temperature of 273 K and determine at what pressure the balloon will burst. (Assume the balloon to be in the shape of a sphere.) This is confusing. It doesn't look like any gas laws I know!

Answer 1

See the sentence "Assume the balloon to be in the shape of a sphere."?
If the maximum surface area of this balloon is 1257 cm^2, its maximum radius is sqrt(1257 cm^2/(4*pi)) = 10.00cm, and thus its maximum volume is 4*pi*r^3/3 = 4.189L
Let "_i" indicate the initial state and "_f" the final state, we have:
759*3.2/292 = P_i*V_i /T_i = P_f*V_f /T_f = P_f*4.189/ 273
Therefore P_f = 759*3.2*273/(292*4.189) = 542 (torr)

Answer 2

First determine the volume of a sphere having a surface area of 1257 cm^2.
1257 cm^2 = 4 pi r^2
1257/(4 pi) = r^2
100 = r^2
r=10 cm
V= (4/3) pi r^3 = 4,189 cm^3 = 4.19 liters

Now it is a gas law problem...at what pressure will the 3.2 L of He expand to a volume of 4.19 liters?

PV/T = pv/t
759*3.2/292=p*4.19/273
p=542 torr

Answer 3

this question makes use of boyle's law that's P1V1=P2V2 a million) organize the understand-the kind you have got P1= a million.08 atm V1=5.00 L P2= ? V2= 10.0 L 2) plug those into the boyle's regulation formula (a million.08 atm) (5.00 L) = (P2)(10.0 L) 3) multiply and settle on on your respond: a million.08 x 5.00 = 5.4, divide 5.4 via 10.0L which equals 0.fifty 4 P2= 0.fifty 4 is your maximum suitable answer distinctive gas criminal rules are: charles regulation - V1/T1= V2/T2 (volume over temperature) gay-lussac - P1/T1=P2/T2 (stress over temperature) perfect gas - PV=nRT (P=stress. V=volume, n=form of moles of gas, R= gas usual), T=temperature