In: Chemistry
A sample of 11.8 liters of an ideal gas at 24.0°C and 725 torr is compressed and heated so that the volume is 6.6 liters and the temperature is 73.0°C. What is the pressure in the container?
moles of gas (n) = PV/RT
with,
P = 725/760 = 0.954 atm
V = 11.8 L
R = gas constant
T = 273 + 24 = 294 K
we get,
moles of gas (n) = 0.954 x 11.8/0.08205 x 294 = 0.47 mol
when, volume is changed to 6.6 L and temperature to 273 + 73 = 346 K
Pressure in the container = nRT/V
= 0.47 x 0.08205 x 346/6.6
= 2.02 atm