Question

A gas occupying 2560 ml at 756 mm Hg pressure at standard temperature is transferred to a 4.50 L container , where pressure is 0.25 atm. What must the temperature be for the gas in the new container to have this pressure ?

Answer 1

121.2 K

Explanation:

P1V1 / T1 = P2V2 / T2

T2 = P2V2T1 / P1V1

P1, V1, T1, P2, V2 are the known quantities

T2 is the unknown quantity.

Standard temperature, T1 = 273 K

Volume, V1 = 2560 ml is converted to litres as 2.56 L

Pressure, P1 = 756 mm Hg is converted into atm as 0.99 atm

P2 = 0.25 atm and V2 = 4.50 L

Now we have to insert these values in the above equation 2 we will get the temperature, T2 as,

T2 = $\frac{0.25 atm \times 4.50 L \times 273K}{ 0.99 atm \times 2.56 L}$

= 121.2 K