Question

A flask of fixed volume contains 1.0 mole of gaseous carbon dioxide and 88 g of solid carbon dioxide. The original pressure and temperature in the flask is 1.0 atm and 300. K. All of the solid carbon dioxide sublimes. The final pressure in the flask is 2.5 atm. What is the final temperature?

Answer 1

the final temperature is 250 K

Step-by-step explanation:

The computation of the final temperature is as follows:

PV = nRT

V1 = n1RT1 ÷ P1

And,

V2 = n2RT2 ÷ P2

n1T1 ÷ P1 = n2T2 ÷ P2

(1 × 300) ÷ 1 = (3 × T2) ÷ 2.5

T2 = (1 × 300 × 2.5) ÷ (1 × 3)

= 250 K

hence, the final temperature is 250 K

We simply applied the above formula so that the correct value could come

And, the same is to be considered