A 2.0 L cannister contains a mixture of nitrogen, oxygen and argon at 4.60 atm. If the abundance of nitrogen and oxygen are 24.38 % and 1 % respectively, then determine the partial pressure of the argon in kPa.
Question
A 2.0 L cannister contains a mixture of nitrogen, oxygen and argon at 4.60 atm. If the abundance of nitrogen and oxygen are 24.38 % and 1 % respectively, then determine the partial pressure of the argon in kPa.
Solution
Sure, here are the steps to solve this problem:
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First, we need to convert the total pressure from atm to kPa because the question asks for the answer in kPa. We know that 1 atm = 101.325 kPa. So, 4.60 atm = 4.60 * 101.325 = 466.095 kPa.
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Next, we need to find the partial pressures of nitrogen and oxygen. We know that the partial pressure of a gas in a mixture is given by the total pressure times the fraction of the total pressure that the gas contributes.
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The fraction of the total pressure that nitrogen contributes is 24.38/100 = 0.2438. So, the partial pressure of nitrogen = 0.2438 * 466.095 = 113.6 kPa.
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Similarly, the fraction of the total pressure that oxygen contributes is 1/100 = 0.01. So, the partial pressure of oxygen = 0.01 * 466.095 = 4.66 kPa.
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Finally, we can find the partial pressure of argon by subtracting the partial pressures of nitrogen and oxygen from the total pressure. So, the partial pressure of argon = 466.095 - 113.6 - 4.66 = 347.835 kPa.
So, the partial pressure of argon in the canister is 347.835 kPa.
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