A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 21 °C is 1.16 atm, what is the partial pressure of nitrogen? The vapor pressure of water at 21 °C is 18.7 mmHg.
I set up an equation according to Dalton's Law of partial pressure ---> 1.16= P1+18.7
I keep getting the answer wrong and need help.
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To solve this problem, you correctly set up an equation according to Dalton's Law of partial pressure. However, there seems to be a mistake in the equation you wrote.
According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas. In this case, the total pressure (1.16 atm) consists of the partial pressure of nitrogen gas, P(N2), and the partial pressure of water vapor, P(H2O).
So the correct equation should be: 1.16 atm = P(N2) + P(H2O)
Given that the vapor pressure of water at 21°C is 18.7 mmHg, you need to convert this to atm for consistency. To convert mmHg to atm, you divide by 760, which is the conversion factor.
So, vapor pressure of water = 18.7 mmHg / 760 mmHg/atm = 0.0246 atm
Now, you can rewrite the equation: 1.16 atm = P(N2) + 0.0246 atm
To find the partial pressure of nitrogen, simply subtract the vapor pressure of water from the total pressure:
P(N2) = 1.16 atm - 0.0246 atm
P(N2) = 1.1354 atm
Therefore, the partial pressure of nitrogen in the mixture at 21°C is approximately 1.1354 atm.