Question

A flask of fixed volume contains 1.00 mole of gaseous carbon dioxide and 88.0 g of solid carbon dioxide. the original pressure and temperature in the flask is 1.00 atm and 300. k. all of the solid carbon dioxide sublimes. the final pressure in the flask is 2.75 atm. what is the final temperature in kelvins? assume the solid carbon dioxide takes up negligible volume.

Answer 1

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Answer 2

Answer: The final temperature of the system is 825 K

Step-by-step explanation:

To calculate the final temperature, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant volume.

Mathematically,

`(P_1)/(T_1)=(P_2)/(T_2)` (at constant volume)

where,

`P_1\text{ and }T_1` are the initial pressure and temperature of the gas.

`P_2\text{ and }T_2` are the final pressure and temperature of the gas.

We are given:

`P_1=1.00atm\\T_1=300K\\P_2=2.75atm\\T_2=?K`

Putting values in above equation, we get:

`(1.00atm)/(300K)=(2.75atm)/(T_2)\\\\T_2=(2.75* 300)/(1.00)=825K`

Hence, the final temperature of the system is 825 K