Question

In: Chemistry

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g...

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total pressure of the mixture is 3.05 atm, what is the partial pressure of each component?

Solutions

Expert Solution

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total

moles of N2 = mass / molar mass = 8.23 / 28

                  = 0.294

moles of H2 = 8.80 / 2 = 4.40

moles of NH3 = 6.96 / 17 = 0.409

total moles = 0.294 + 4.40 + 0.409 = 5.103

mole fraction of N2 = moles of N2 / total moles = 0.294 / 5.103

                                = 0.0576

mole fraction of H2 = 4.40 / 5.103 = 0.862

mole fraction of NH3 = 0.409 / 5.103 = 0.080

Partial pressure of N2 = mole fraction of N2 x total pressure

                                    = 0.0576 x 3.05

                                    = 0.176 atm

partial pressure of H2 = mole fraction of H2 x total pressure

                                   = 0.862 x 3.05

                                   = 2.63 atm

partial pressure of NH3 = mole fraction of NH3 x total pressure

                                      = 0.080 x 3.05

                                      = 0.244

queen_honey_blossom answered 3 weeks ago
Next > < Previous

Related Solutions

A gaseous mixture contains 421.0 Torr of H2(g), 392.9 Torr of N2(g), and 68.1 Torr of...
A gaseous mixture contains 421.0 Torr of H2(g), 392.9 Torr of N2(g), and 68.1 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.
A gaseous mixture contains 413.0 Torr of H2(g), 391.5 Torr of N2(g), and 65.7 Torr of...
A gaseous mixture contains 413.0 Torr of H2(g), 391.5 Torr of N2(g), and 65.7 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.
An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2....
An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2. At this temperature, Kc for the reation N2(g)+3H2(g) <> 2NH3(g) is 0.29. What is the concentration of NH3?
A gas mixture contains the following gases at the indicated partial pressures: N2, 310. torr ;...
A gas mixture contains the following gases at the indicated partial pressures: N2, 310. torr ; O2, 144 torr ; and He, 225 torr. 1. What mass of each gas is present in a 2.85 L sample of this mixture at 25.0 ∘C?
A gas mixture contains the following gases at the indicated partial pressures: N2, 310. torr ;...
A gas mixture contains the following gases at the indicated partial pressures: N2, 310. torr ; O2, 144 torr ; and He, 225 torr. 1. What mass of each gas is present in a 2.85 L sample of this mixture at 25.0 ∘C?
A gas mixture contains 0.650 mol of N2, 0.100 mol of H2, and 0.400 mol of...
A gas mixture contains 0.650 mol of N2, 0.100 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 11.0 L vessel at 27.00°C. 1) Total Pressure: 2.57 atm 2) Pressure of H2: ____ atm 3) Pressure of N2: ____ atm 4) Pressure of CH4: ___ atm
A gas mixture contains 1.25 g N2 and 0.84 g O2 in a 1.53-L container at...
A gas mixture contains 1.25 g N2 and 0.84 g O2 in a 1.53-L container at 14 ∘C. A.) Calculate the mole fraction of N2. B.) Calculate the mole fraction of O2. C.) Calculate the partial pressure of N2. D.) Calculate the partial pressure of O2.
- 25.0-L tank contains 295 g N2, 135 g O2, and 24.0 He gases. Calculate the...
- 25.0-L tank contains 295 g N2, 135 g O2, and 24.0 He gases. Calculate the partial pressure of each gas and the total gas pressure at 20.0oC.          (Answer: PN2 = 10.1 atm; PO2 = 4.06 atm; PHe = 5.77 atm; Ptotal = 19.9 atm) - A 5.0-gallon gas tank contains N2 and H2 gas, such that the partial pressure of H2 is three times that of N2 gas. If the total gas pressure is 2.4 atm at 25oC,...
Suppose 13.85 g N2 and 1.88 g H2 are combined in a 2.50 L flask. At equilibrium, we find that the flask still contains 7.00 g N2.
Consider the reaction: N2 + 3H2 ↔ 2NH3             Suppose 13.85 g N2 and 1.88 g H2 are combined in a 2.50 L flask. At equilibrium, we find that the flask still contains 7.00 g N2.             a.         Calculate the equilibrium concentrations of N2, H2, and NH3.             b.         Calculate KC.
Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts...
Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts with 18 g of H2(g). d. What is the limiting reactant? e. When the reaction is complete, how many grams of NH3(g) are produced? f. When the reaction is complete, how many grams of N2(g) remain? g. When the reaction is complete, how many grams of H2(g) remain? h. If the reaction actually produced 55 g of NH3(g), what is the percent yield?
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT