Question

A vessel of 120ml capacity contain amount at gass at 35c and 1.2bar pressure .the gas is transferred to another vessel of volume 180ml at 35c .what would be it's pressure

Answer 1

Given:

• Initial pressure(p1) = 1.2 bar.

• Initial volume(v1) = 120 ml.

• Initial temerature(T1) = 35° C

• Final volume(v2) = 180 ml.

• Final temperature(T2) = 35° C

To find:

The final pressure of the gas (p2)

Solution:

Initial pressure(p1) = 1.2 bar.

Initial volume(v1) = 120 ml.

Initial temerature(T1) = 35° C

                                 = (35 +273.15) K

                                 = 308.15 K.

Final volume(v2) = 180 ml.

Final temperature(T2) = 35° C

                                    = (35+273.15) K

                                    = 308.15 K

Final pressure(p2) =?

From the ideal gas law equation we get that,

$\dfrac{p1v1}{T1} = \dfrac{p2v2}{T2}$

⇒ (1.2×120)/308.15 = (p2×180)/ 308.15

⇒ (1.2×120) = (p2×180)

⇒(p2×180) = (1.2×120)

⇒(p2×180) = 144

⇒ p2 = (144÷180)

⇒ p2 = 0.8 bar.

∴ The final pressure of the gas will be 0.8 bar.

Answer:

             The pressure of the gas will be 0.8 bar.