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 gas is, 825 K

Explanation :

According to the Gay-Lussac's law, the pressure of the gas is directly proportional to the temperature if the gas ate constant volume of number of moles of gas.

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 1 atm

$P_2$ = final pressure of gas = 2.75 atm

$T_1$ = initial temperature of gas = 300 K

$T_2$ = final temperature of gas = ?

Now put all the given values in the above equation, we get the final temperature of gas.

$\frac{1atm}{300K}=\frac{2.75atm}{T_2}$

$T_2=825K$

Therefore, the final temperature of the gas is, 825 K