Question

Chlorine gas occupies
of 1. 2 litres at 720 torr pressure
What volume will it occupy at 10 atm pressure

Answer 1

Answer:

Well,

1 Torr = 1 mm Hg

...

Explanation:

And

1

⋅

a

t

m

≡

760

⋅

m

m

⋅

H

g

or rather

1

⋅

a

t

m

will support a column of mercury that is

760

⋅

m

m

high...and I truly hope you have seen such a column because the health and safety commissars at my establishment have declared the mercury column counter-revolutionary.

And we simply apply old

Boyles' Law..

P

1

V

1

=

P

2

V

2

We solve for

V

2

=

P

1

V

1

P

2

=

1.20

⋅

L

×

720

⋅

m

m

⋅

H

g

760

⋅

m

m

⋅

H

g

⋅

a

t

m

−

1

760

⋅

m

m

⋅

H

g

760

⋅

m

m

⋅

H

g

⋅

a

t

m

−

1

≡

1.14

⋅

L

...the VOLUME has reduced because we INCREASED the PRESSURE

Answer 2

Answer:

If temperature is constant then for a gas

PV = constant

P

1

V

1

=

P

2

V

2

V

2

=

P

1

V

1

P

2

=

720

torr

×

1.2 L

760

torr

=

1.14 L

Note: 1 atm = 760 torr