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?

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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.**

the above is wrong, the answer is 54.27cm cube

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