Question

A sample of O2 under 2.00 atm occupies 500 ml at 25.0˚C. What pressure will the sample have at 0.0˚C ?

Answer 1

In this question we will use the ideal gas equation.

P

1

x

V

1

/

T

1

=

P

2

x

V

2

/

T

2

P

1

= 2 atm

V

1

= 500 mL

T

1

= 25 + 273 = 298 K

P

2

= ?

V

2

= 500 mL

T

2

= 0 + 273 = 273 K

substituting values;

2 atm x 500 mL / 298 K =

P

2

x 500 mL / 273

rearranging we get,

1000 atm mL x 273 K / 500 mL x 298 K =

P

2

P

2

= 1.83 atm.

Answer 2

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