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Answer :
The pressure of oxygen gas in a mixture of nitrogen and helium is to be determined.
The three gases are present in a 2.00 liter container, and their individual pressures are known. The total pressure exerted by the three gases in the container is also given.
In order to determine the pressure of the oxygen gas, we will need to apply Dalton's law of partial pressures. According to this law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. Mathematically, we can express this as:
P_total = P_1 + P_2 + P_3
where P_total is the total pressure, and P_1, P_2, and P_3 are the partial pressures of the gases.
In the given problem, we know the partial pressures of nitrogen and helium, and the total pressure of the mixture. Therefore, we can write:
P_total = P_N2 + P_He + P_O2
Substituting the values given in the problem, we get:
1173.99 torr = 215.91 torr + 53.46 torr + P_O2
Solving for P_O2, we get:
P_O2 = P_total - P_N2 - P_He
P_O2 = 1173.99 torr - 215.91 torr - 53.46 torr
P_O2 = 904.62 torr
Therefore, the pressure of the oxygen gas in the mixture is 904.62 torr.
To learn more about oxygen click brainly.com/question/24259144
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