Question

Neon gas occupies a metal container of 5.5 L at STP (273 K, 1 atm). The volume of the metal container cannot be changed. What will happen to the pressure if the temperature rises to 300K? A. It will fall to 0.7 atm. B. It will fall to 0.9 atm. C. It will rise to 1.1 atm. D. It will rise to 1.3 atm.

Answer 1

C. It will rise to 1.1 atm. 

Answer 2

Answer: C. It will rise to 1.1 atm

Step-by-step explanation:

Gay-Lussac's Law: This law states that pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

`P\propto T` (At constant volume and number of moles)

`(P_1)/(T_1)=(P_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 1 atm

`P_2` = final pressure of gas = ?

`T_1` = initial temperature of gas =
`273K`

`T_2` = final temperature of gas = 300 K

`(1)/(273)=(P_2)/(300)`

`P_2=1.1atm`

Thus the final pressure will be 1.1 atm