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?

the final temperature is 250 K

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

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

the ratio of the conjugate base to the acid required to attain the desired ph.