A vessel of 120 mL capacity contains a certain amount of gas at temperature `35^(@)C` and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at temperature `35^(@)C`, What would be its pressure ?

Explanation

When fixed mass of any gas is poured to one container to another container then its pressure, volume and temperature is as under.
Container - 1st : Initial volume `(V_(1))=120` mL
Initial pressure `(p_(1))=1.2` bar
Temperature `(T) = 35^(@)C`
Container - 2nd : Final volume `(V_(2))=180` mL
Temperature (T) `= 35^(@)C`
Final pressure `(p_(2))=(?)`
Temperature is constant at `35^(@)C` and mass of gas is constant so according to Boyle.s law.
`p_(1)V_(1)=p_(2)V_(2)`
`therefore p_(2)=(p_(1)V_(1))/(V_(2))=(("1.2 bar")xx(120 mL))/(180 mL)=0.8` bar
Pressure of container - 2nd would be 0.8 bar.