We can use the combined gas law to solve for the new pressure:
(P1 x V1) / (T1) = (P2 x V2) / (T2)
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.
Plugging in the given values:
P1 = 700.4 torr
V1 = 2.5 L
T1 = 31.4 + 273.15 = 304.55 K
V2 = 0.20 L
T2 = 663.3 + 273.15 = 936.45 K
(P1 x V1) / (T1) = (P2 x V2) / (T2)
(700.4 torr x 2.5 L) / (304.55 K) = (P2 x 0.20 L) / (936.45 K)
Simplifying:
P2 = (700.4 torr x 2.5 L x 936.45 K) / (304.55 K x 0.20 L)
= 43,330.0 torr
Converting to atmospheres:
P2 = 43,330.0 torr / 760 torr/atm
= 57.0 atm
Therefore, the new pressure of the gas is 57.0 atm.