Question

A sample of ammonia gas is placed in a container of volume 250 ml exerts a pressure of 72 cmHg. The gas is transferred to a 400 ml. the container
at the same temperature.what will be its pressure ?​

Answer 1

Answer:

Explanation:

Given: P  1  =745 mm Hg

V  1  =250 ml  

V  2  =200 ml

∴ By Boyle's law as the temperature is constant.

P  2  = ​P  1  V  1 = 745×250   =  931.25 mm Hg

         V  2             200  

Additional pressure required =931.25−745=186.25 mm

Answer 2

Answer:

468.75mmHg or46.875cmHg or 0.616atm

Explanation:

given that,

V1=250ml

P1=75cmHg=750mmHg (1cm=10mm)

V2=400ml

P2=?

we knot that,

a/c to Boyle's law,

P1V1=P2V2

so,750*250=400*P2

P2=750*250/400

P2=468.75mmHg

=46.875cmHg

=0.616atm

(1atm=760mmHg)