Solution:

Given:
Mass of gas (m) = 20 g
Volume of vessel (V) = 22.5 L
Initial temperature (T1) = 0°C = 273 K
Final temperature (T2) = 150°C = 423 K

We need to find the mass of gas that escapes from the vessel when the temperature is raised to 150°C at constant pressure.

Using the ideal gas equation, PV = nRT, we can calculate the number of moles (n) of gas present in the vessel at initial conditions.

n = PV/RT1
where,
P = pressure (taken as constant)
R = gas constant = 8.31 J/mol K

Substituting the given values, we get:
n = (P x 22.5)/(8.31 x 273) mol

We also know that the mass of gas (m) can be expressed in terms of the number of moles (n) and molar mass (M) of the gas as:

m = n x M

Rearranging the above equation, we get:
n = m/M

Substituting the given values, we get:
n = 20/ M mol

Equating the two expressions for n, we get:
(P x 22.5)/(8.31 x 273) = 20/M
Solving for M, we get:
M = (20 x 8.31 x 273)/(P x 22.5)

Now, at the final temperature of 150°C (423 K), the volume of the vessel remains constant. Therefore, the pressure of the gas also remains constant.

Using the ideal gas equation again, we can calculate the number of moles of gas present in the vessel at the final temperature:

n' = PV/RT2

Substituting the given values, we get:
n' = (P x 22.5)/(8.31 x 423) mol

The mass of gas that remains in the vessel at the final temperature is:

m' = n' x M

Substituting the value of n' and M, we get:
m' = (P x 22.5 x 20)/(8.31 x 423) g

Therefore, the mass of gas that escapes from the vessel is:
m - m' = 20 - (P x 22.5 x 20)/(8.31 x 423) g

We cannot calculate the exact value of the pressure without additional information. However, we can assume that the pressure is constant and cancel it out to get an approximate answer as follows:

m - m' = 20 - (1/4)g
(This assumes that the pressure remains constant at approximately 1 atm)

Therefore, the approximate mass of gas that escapes from the vessel is 20 - (1/4) g = 19.75 g.

Hence, the answer is 19.75 g (approximate).

Any one please answer this and help me