The flasks illustrate a mixture of diatomic nitrogen (N2) and oxygen (O2) molecu

Question

The flasks illustrate a mixture of diatomic nitrogen (N2) and oxygen (O2) molecules. Each flask has the same volume and temperature. The nitrogen molecules are shown in blue and the oxygen molecules are shown in red.

Part 1) Which flask has the greatest partial pressure of nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. _______

Part 2) Which flask has the greatest partial pressure of oxygen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. _______

Part 3) Which flask has equal partial pressures of oxygen and nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter for the flask. _______

Part 4) Given the identical total pressures for each flask, which flask has the highest temperature? Enter the letter for the flask. ______

Part 5) Flask (a) has an initial partial pressure of 578 torr and a temperature of 400.0 K. What is the partial pressure of the flask at 200.0 K? Assume volume and the number of moles remain constant. _____ torr?

Explanation / Answer

Part 1) Which flask has the greatest partial pressure of nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. _______ the bottle with MOST BLUE particles --> this must be " B" with 6 particles of N2

Part 2) Which flask has the greatest partial pressure of oxygen, assuming that each flask has a total pressure of 1 atm? Enter the letter of the flask. _______this must be "D" since it has 6 particles of O2

Part 3) Which flask has equal partial pressures of oxygen and nitrogen, assuming that each flask has a total pressure of 1 atm? Enter the letter for the flask. _______equal mounts of red=blue --> A only

Part 4) Given the identical total pressures for each flask, which flask has the highest temperature? Enter the letter for the flask. ______highest T is given by highest P --> A,B,D only

Part 5) Flask (a) has an initial partial pressure of 578 torr and a temperature of 400.0 K. What is the partial pressure of the flask at 200.0 K? Assume volume and the number of moles remain constant. _____ torr?

P1/T1 = P2/T2

P2 = T2/T1 * P1 = 200/400*578 = 289 torr

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