At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 ...

Question

At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 L. (Section 10.4) (b) Looking at Figure 18.1, we see that the temperature is lower at 85 km altitude than at 50 km. Does this mean that one mole of an ideal gas would occupy less volume at 85 km than at 50 km? Explain.

Accepted Answer

Hey everyone today, we're being asked under which conditions with one mole of an ideal gas occupy less volume. So right off the bat, we're dealing with an ideal gas and were given the temperature and pressure for the different conditions. So using this, we can go ahead and actually use the ideal gas formula P. V. Sorry, P V is equal to N R. T. Where and is the number of moles are the constant T. Is temperature volume and P is pressure. Now, in this case we're dealing with one mole of gas that isn't changing and our is also the same. But the three the two conditions that are changing are the temperature and the pressure. So essentially we're dealing with P V C T as the N R constant here. So as such, to determine which one will have less volume, we can go ahead and solve for volume, which will be temperature divided by pressure. So now, with this knowledge, we can go ahead and take a look at the two different conditions. 1st, looking at a, we have P is equal to 0.74, A. T. M and T. Is 250 kelvin. So, T by P therefore becomes uh 2 50 divided by 0.74, which equals 337.84. That is our volume in this case, and we don't really need to put a unit after it. It is just an abstract number at the moment for B four B, We have 180 Kelvin. So it's T by P. So it's 180 Kelvin divided by 0. atmospheres, which will give us a value of 562.50. So the volume that it occupies will be 562.5. Whatever units as such, we can clearly see that less volume will be occupied under the conditions of the first uh first data set with the pressure at 0.74 a t. M. And a temperature of 2 50 kelvin. Therefore, this will lock. This specific set of conditions will allow us to occupy less volume with one mole of ideal gas. I hope this helps. And I look forward to seeing you all in the next one.

At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 L. (Section 10.4) (b) Looking at Figure 18.1, we see that the temperature is lower at 85 km altitude than at 50 km. Does this mean that one mole of an ideal gas would occupy less volume at 85 km than at 50 km? Explain.

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