Answer:
180 Torr.
Step-by-step explanation:
Step 1:
Data obtained from the question. This include the following:
Initial temperature (T1) = 127 °C
Initial volume (V1) = 400 mL
Initial pressure ( P1) = 120 Torr
Final volume (V2) = 200 mL
Final temperature (T2) = 27 °C
Final pressure (P2) =..?
Step 2:
Conversion of celsius temperature to Kelvin temperature.
This is illustrated below:
Temperature (Kelvin) = Temperature (celsius) + 273
T(K) = T(°C) + 273
Initial temperature (T1) = 127 °C
Initial temperature (T1) = 127 °C + 273 = 400 K
Final temperature (T2) = 27 °C
Final temperature (T2) = 27 °C + 273 = 300 K
Step 3:
Determination of the final pressure.
This can be obtained by using the general gas equation as shown below:
Initial temperature (T1) = 400 K
Initial volume (V1) = 400 mL
Initial pressure ( P1) = 120 Torr
Final volume (V2) = 200 mL
Final temperature (T2) = 300 K
Final pressure (P2) =..?
P1V1/T1 = P2V2/T2
120 x 400/400 = P2 x 200/300
120 = P2 x 2/3
Cross multiply
P2 x 2 = 120 x 3
Divide both side by 2
P2 = (120 x 3)/2
P2 = 180 Torr.
Therefore, the new pressure exerted by the gas is 180 Torr.