Posted by paro on Monday, April 5, 2010 at 1:23pm.
0.11 mol of argon gas is admitted to an evacuated 50cm^3 container at 10 degree C. The gas then undergoes an isothermal expansion to a volume of 200cm^3.
What is the final pressure of the gas?

physics  drwls, Monday, April 5, 2010 at 3:42pm
In isothermal expansions, the product
P*V = a constant. Therefore
P2/P1 = V1/V2 = 50/200 = 1/4
Since you were not told the initial pressure P1, you will have to use the perfect gas law and the information given.
0.11 moles at STP (1 atm and 273K) occupies 0.11*22.4 = 2.46 liters. At 10C (283K) it would occupy 2.55 liters. Since the initial volume is only 50 cm^3 = 0.05 l, the initial pressure must be
P1 = 2.55/0.05 = 51 atm.
The final pressure is 1/4 of that.
You could also have used P = nRT/V to get the initial pressure. Personally I find it easier to remember that 1 mole is 22.4 liters at STP. There are too many values of R, with different units, to try to remember.
Answer This Question
Related Questions
 Physics  Assume that 0.10 mol of argon gas is admitted to an evacuated 50 cm3 ...
 physics  .10 mol of Argon gas is admitted to an evacuated 50cm cubed container ...
 Physics  0.75 mol of argon gas is admitted to an evacuated 40 cm^{3} container ...
 Physics Help  0.30 mol of argon gas is admitted to an evacuated 50cm^3 ...
 Physics  0.490 mol of argon gas is admitted to an evacuated 50.0 cm^3 container...
 physics  0.75 mol of argon gas is admitted to an evacuated 40 cm^{3} container ...
 physics  A monatomic ideal gas (Cv = 3/2 R) undergoes an isothermal expansion ...
 Physics  0.75 mol of argon gas is admitted to an evacuated 40 cm^{3} container ...
 Physics I  A container of volume 0.71 m3 contains 1 mol of argon gas at 27&#...
 physics vry urgent  An ideal monatomic gas initially has a temperature of 333 ...
More Related Questions