A gas syringe contains 50 cm^3 of oxygen gas at 20 deg C. If the temperature was increased to 45 deg C, what would be the volume occupied by this...gas, assuming constant pressure throughout?
We use the ideal gas law here. PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature. Initially the gas syringe contains 50 cm^3 of oxygen gas. The initial temperature is 20+ 273 = 293 K.The final temperature is 273+ 45 = 318 K.
Let's rewrite PV=nRT as R = PV/ nT.
As R is a constant it remains the same for both the temperatures.
=> P*50 / n*273 = P*V/ n*318
Now the pressure is also the same throughout
=> 50 / 273 = V / 318
=> V = 318*50 / 273
=> V = 58.24 cm^3
Therefore the volume occupied changes to 58.24 cm^3 when the temperature is raised from 20 to 45 deg C.