Oxygen, Nitrogen, and hydrogen are in a 6-liter container. The total pressure in the container is 8.00 atm. If the oxygen is 3.00 atm and the nitrogen is 2.50 torr, what is the partial pressure of the hydrogen?

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This problem can be solved using Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases:

`P_(Total) = P_A + P_B + P_C +....`

In this case,

`8.00 atm = P_(Total)...

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This problem can be solved using Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases:

`P_(Total) = P_A + P_B + P_C +....`

In this case,

`8.00 atm = P_(Total) = P_O_2 + P_N_2 + P_H_2`

so

`P_H_2 =P_(Total) - P_O_2 - P_N_2`

The partial pressure of nitrogen must be converted to atmospheres to be consistent with the other two pressure values:

2.50 torr x (1 atm/760 torr) = 0.00329 atm

The partial pressure of hydrogen is:

8.00 atm - 3.00 atm - 0.00329 atm = 4.9967 atm

Rounded to 3 significant digits: 5.00 atm

The partial pressure of an individual gas in a gas mixture is the pressure the gas would exert if it was the only gas in the container. When a gas mixture behaves ideally, each gas in the mixture obeys the ideal gas law independently, regardless of other gases present.

 

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