Acontainer holds oxygen, hydrogen and nitrogen gas. the nitrogen gas has a partial pressure of 0.88 atm, while occupying 15% of the container’s volume. if the oxygen gas occupies 57% of the container’s volume, what is the partial pressure of the hydrogen gas in the container? a. 0.88 atm b. 1.64 atm c. 3.34 atm

The partial pressure of hydrogen gas = 1.64 atm

Explanation:

Step 1: Data given

partial pressure of nitrogen = 0.88 atm

Nitrogen occupies 15% of the volume (Let's assume the volume is 1L)

Oxygen gas occupies 57 % of the volume

Step 2: Calculate % volume of hydrogen

100 % - 15% - 57 % = 28 %

Step 2:

P1/V1 = P2/V2

⇒ with p1 = the partial pressure of nitrogen = 0.88 atm

⇒ with V1 = the volme occupied by nitrogen = 15% ( assume 0.15 L)

⇒ with P2 = the partial pressure of hydrogen = TO BE DETERMINED

⇒ with V2 = the volume occupied by hydrogen = 28 % = 0.28 L

0.88/ 0.15 = X/0.28

X = 1.64 atm

The partial pressure of hydrogen gas = 1.64 atm

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.