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

Answer:

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

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:

$\frac{P_1}{T_1}=\frac{P_2}{T2}$

$P_2=\frac{750 torr\times 450 K}{300 K}=1,125 torr$

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