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?
1.650atm
0.825atm
0.413atm
0.275atm
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𝐏𝐯 = 𝐧𝐑𝐓
𝐯, 𝐑 𝐚𝐧𝐝 𝐓 𝐚𝐫𝐞 𝐜𝐨𝐧𝐬𝐭𝐚𝐧𝐭
𝐏/𝐧 = 𝐏'/𝐧'
𝐧' = 0.5𝐧
0.825/𝐧 = 𝐏'/0.5𝐧
𝐏' = 0.4125 𝐚𝐭𝐦. 𝐂
My school your answer is wrong. Please study the question very well andake corrections. First the volume of oxygen was not given but what was given is the volume of the container. And secondly, the volume of the container was not halved but rather is was the QUANTITY OF OXYGEN. So as a gas if the container is the same and you take away half of the Oxygen present then it means the volume of the container has been doubled technically speaking and the pressure will be halved. Because you cannot reduce the quantity of oxygen and expect the pressure to reduce. So please take note!
in this case since the temperature is not specified to remain constant, we can't assume it does. We'd need to use the combined gas law, which incorporates Boyle's law, Charles's law, and Gay-Lussac's law.
However, for this particular problem, since only the volume is changing while the temperature and the quantity of gas are not specified to change, Boyle's law can still be applied. So, the pressure exerted by the remaining gas would be twice the original pressure, hence the correct answer is still A. 1.650 atm.
Using the ideal gas law, PV = nRT, we can solve for the initial number of moles of oxygen (n):
PV = nRT
(0.825 atm)(2.76 L) = n(8.3145 L atm/mol K)(300 K)
n = 0.00852 mol
If the quantity of oxygen is reduced by half, the new number of moles is:
n = 0.00852 mol / 2 = 0.00426 mol
We can now use the ideal gas law again to find the new pressure:
PV = nRT
P(2.76 L) = (0.00426 mol)(8.3145 L atm/mol K)(300 K)
P = 0.4125 atm
Therefore, the pressure exerted by the remaining gas is 0.4125 atm or 41.25 kPa.
In this question the pressure was reduced by half not the volumn so the answer is C
people it os 0.4125 cos we are dealing with number of molecule and volume of gas(chemical aspect of gas laws) not volume of container (physical aspect or boyles law) and beside its common sence
