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parwana
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A mixture of 5.40 g of N2 and 10.2 g of Kr exerts a pressure of 0.505 atm.
What is the partial pressure, in atm, of Kr?
What is the partial pressure, in atm, of Kr?
parwana said:i got it, i got the mole fraction of Ke and then times thta by total pressure.
Partial pressure is the pressure exerted by an individual gas component in a mixture of gases. It is proportional to the amount of that gas present in the mixture.
Partial pressure can be calculated by multiplying the total pressure of the gas mixture by the mole fraction of the gas component in the mixture. In this case, the partial pressure of Kr would be calculated by multiplying the total pressure (0.505 atm) by the mole fraction of Kr (0.505).
Partial pressure is important because it helps us understand the behavior of gases in mixtures. It is also used to determine the concentration of a specific gas in a mixture and to predict how gases will move in and out of a system.
The partial pressure of a gas can be affected by changes in temperature, volume, and the amount of the gas present in the mixture.
The partial pressure of Kr in the N2/Kr mixture (0.505 atm) is equal to the total pressure of the gas mixture, while the partial pressure of N2 would be lower since it is present in a smaller amount. In this case, the partial pressure of N2 would be around 0.495 atm.