A mixture of nitrogen (N₂) and helium has a volume of 250 mL at 3...

Question

A mixture of nitrogen (N₂) and helium has a volume of 250 mL at 30 °C and a total pressure of 745 mmHg. (8.5, 8.6, 8.7)

a. If the partial pressure of helium is 32 mmHg, what is the partial pressure of the nitrogen?

Accepted Answer

Welcome back, everyone. A 500 mL vessel contains a mixture of neon gas and chlorine gas. The total pressure of the mixture at 28 Celsius is 7 45 millimeters of mercury. Calculate the partial pressure of chlorine. If neon has a partial pressure of 148 millimeters of mercury, we're going to begin by recalling that. Dalton's law describes our total pressure to which is equal to the sum of our partial pressures of our non reacting gasses. So we would have our partial pressure of our first gas plus the partial pressure of our second gas. And in our equation, we only have two gasses described. So we have the pressure of gas one and our partial pressure of gas two. So let's actually plug in what gas one would be. And we'll assign that to neon gas. And for gas two, we would assign chlorine gas. Now, from the prompt were given our total pressure of millimeters of mercury. So we would set that equal to our pressure of neon gas. Our partial pressure of neon gas, which is given as 148 millimeters of mercury, which is added to our partial pressure of our chlorine gas. And so we're going to need to figure out the partial pressure of chlorine based on this given information. So we're going to need to isolate for our pressure of chlorine gas by subtracting both sides from 148 millimeters of mercury of neon gas on both sides of our equation. This will allow us to cancel out 148 millimeters of mercury from the right hand side of our equation. And as a result, we'll find that our pressure of our chlorine gas, partial pressure of chlorine gas is equal to the result of our difference on the left being a value of millimeters of mercury. And this would be our final answer as the partial pressure of chlorine gas given neons partial pressure and the total partial or the total pressure of our mixture in our vessel. So again, our partial pressure of chlorine is equal to 597 millimeters of mercury. I hope this made sense and let us know if you have any questions.

A mixture of nitrogen (N₂) and helium has a volume of 250 mL at 30 °C and a total pressure of 745 mmHg. (8.5, 8.6, 8.7) a. If the partial pressure of helium is 32 mmHg, what is the partial pressure of the nitrogen?

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