If the quantity of oxygen occupying 2.76L container at a pressure of 0.825 atm and 300k is reduced by one-half, what is the pressure exerted by the remaining gas?
Using the combined gas law formula,
In this problem, the oxygen is contained in a 2.76 L container at a temperature of 300 K. Since the gas remains in the same container and the temperature is not stated to change, both the volume( V) and the temperature (T) are constant.
The Ideal Gas Law is defined as: PV = nRT
Since the quantity of gas is reduced by one-half ( n\(_2\) = \(\frac{1}{2}\) n\(_1\)), the pressure must also be reduced by one-half.
P\(_2\) = \(\frac{1}{2}\) P\(_1\)
P\(_2\) = \(\frac{0.825}{2}\)
= 0. 4125 atm
Rounding to three decimal places (as provided in the options), the pressure is 0.413 atm.
There is an explanation video available below.
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