In a gaseous mixture, the partial pressures of its component gases are: N_2: 13

Question

In a gaseous mixture, the partial pressures of its component gases are: N_2: 13 atm, NH_3: 5.5 atm, and H_2: 8.5 atm. Calculate the total pressure and the mole fraction of each gas within the mixture. Calcium reacts with water to produce hydrogen gas. Determine the mass of H_2 produced at 25 degree C and 0.967 atm when 525 mL of gas is collected over water. The vapor pr of water at 25 degree C is 23.8 torr. Ca + 2 H_2O rightarrow Ca(OH)_2 + H_2 Calculate the density of NO_2 gas at 0.970 atm and 35 degree C.

Explanation / Answer

) Total pressure is the sum of partial pressures of all its constituent gases

Ptotal = P N2 + P NH3 + P H2

        = 13atm + 5.5atm + 8.5atm = 27atm

Consider a gas A

Partial pressure of A = mole fraction of A* total pressure

So mole fraction of A = partial pressure of A / total pressure

Mole fraction of N2 = 13/27 = 0.481

Mole fraction of NH3 = 5.5/27 = 0.204

Mole fraction of H2 = 8.5/27 = 0.315

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.