From the data in Table 18.1, calculate the partial pressures of carbon dioxide and argon when the total atmospheric pressure is 1.05 bar.

Question

Accepted Answer

hi everyone for this problem we're being asked to calculate the partial pressure of N. O. And K. Are in air at 1.23 bar. If they're more fractions are five times 10 to the negative seven and 1.14 times 10 to the negative six respectively. Okay, so our goal here is to calculate partial pressure were given in the problem. The total pressure and were given the mole fractions. Okay, so let's recall the definition of partial pressure are partial pressure is going to equal our mole fraction times our total pressure. So for our first one are partial pressure of N. O. Is going to equal our mole fraction of N. O. Times are total pressure. So we have all of these values. Let's go ahead and plug them in. Our more fraction for N. O. Is given its 5.0 times 10 to the negative seven. And our total pressure is 1.23 bar. So that means our partial pressure for N. O. Is going to be 6. times 10 to the negative seven bar. Okay, so this is going to be our partial pressure for an O. We multiplied our mull fraction by our total pressure. So for our partial pressure of K. R we're going to use the mole fraction of K. R. Times are total pressure and our mole fraction for K R is 1.14 times 10 to the negative six And our total pressure is 1.23 bar. So that gives us a partial pressure of K. R. Equal to 1. times 10 to the negative six bar. And this is going to be our final answer. These are both of the partial pressures, respectively. That's the end of this problem. I hope this was helpful.

From the data in Table 18.1, calculate the partial pressures of carbon dioxide and argon when the total atmospheric pressure is 1.05 bar.

Verified Solution

Key Concepts

Dalton's Law of Partial Pressures

Mole Fraction

Ideal Gas Law