a flexible container, like a balloon, with an initial volume of 1.0L is occupied by a gas at a pressure 1.5atm at 25 Celsius.what is the...

Gases are measured using three variables:  temperature
(T), pressure (P), and volume (V).

When more than one
variable is changing you use the universal gas law which combines Boyle's Law and
Charles's Law into one general equation.

That equation
is:

(P1 x V1)/T1 = (P2 x 
V2)/T2

where P1, V1 & T1 are initial conditions and
P2,V2,T2 are final conditions.

There are three important
things you need to watch when solving these problems:

1:
make sure the temperature is converted to degrees Kelvin using the formula:  K = 273.15
+ degrees C

2. make sure the units for pressure are the
same for the initial state and final state.  You do not have to change them to kPa
unless that is the units you are asked to use in the final
answer.

3. make sure the units for volume are the same for
the initial and final states.

Once you have done this, put
your known values into the equation above and solv e for the
unknown.

In this problem:

P1 =
1.5 atm

V1 = 1 liter

T1 = 25
degrees C = 298.15 K

P2 = 6
atm

V2 = ?

T2 = 100 degrees C
= 373.15 K

Solving:

(1.5 x
1)/298.15 = (6V2)/373.15

first multiply both sides by
373.15 and you get

(373.15 x 1.5 x1)/298.15 =
6V2

now divide both sides by 6 to find
V2

(373.15 x 1.5 x1)/(298.15 x 6) =
V2

solving you get V2 = .313 liters or 313
mL

Notice that in this case the increased pressure had a
greater effect on the final volume than the increased
temperature.