Question

What pressure must be applied to keep a gas at 750 torr and 300 K at a constant volume of 200 mL if the temperature is raised to 450 K?

Answer 1

p1/t1=p2/t2
750/300=p2/450
p2= 750*450/300
=1125torr

Answer 2

The pressure must be applied at 450 K should be 1,125 torr.

Step-by-step explanation:

At constant volume of 200 mL

Initial pressure exerted by the gas =
`P_1=750 torr`

Initial temperature of the gas =
`T_1=300 K`

Final pressure exerted by the gas =
`P_1=? torr`

Final temperature of the gas =
`T_2=450 K`

Applying Gay Lussac Law:

`(P_1)/(T_1)=(P_2)/(T2)`

`P_2=(750 torr* 450 K)/(300 K)=1,125 torr`

The pressure must be applied at 450 K should be 1,125 torr.