Question

In: Chemistry

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.

Solutions

Expert Solution

PH2    =413 Torr

PN2    = 391.5 Torr

PAr     = 65.7 Torr

Total pressure = PH2 + PN2 + PAr

                         = 413+391.5 +65.7 =870.2 Torr

partial pressure   = mole fraction of gas* total pressure

PH2                   = XH2 * PT

413                    = XH2 *870.2

XH2                     = 413/870.2    = 0.475

PN2                   = XN2 * PT

391.5                 = XN2 *870.2

XN2                    = 391.5/870.2   = 0.45

PAr                   = XAr * PT

65.7                 = XAr *870.2

XAr                   = 65.7/870.2   = 0.0755

queen_honey_blossom answered 1 year 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 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?
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 gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass. What is the...
A gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 385 mmHg ? Express you answer numerically in millimeters of mercury.
5)A gaseous mixture composed of 16.0 g of O2 , 21.0 g of N2, and 16.0...
5)A gaseous mixture composed of 16.0 g of O2 , 21.0 g of N2, and 16.0 g of He at 20.0°C is confined in a 25.0 L container. What is the partial pressure of N2 in this mixture? 6)A gaseous mixture composed of 16.0 g of 2, 21.0 g of N2, and 16.0 g of He at 20.0°C is confined in a 25.0 L container. What is the partial pressure of He in this mixture? 7)Assuming ideal gas behavior, what...
A vessel contains a gaseous mixture of composition by volume 80% H2, and 20% CO.
A vessel contains a gaseous mixture of composition by volume 80% H2, and 20% CO. It is desired that the mixture should be made in the proportion 50% H2 and 50% CO by removing some of the mixture and adding some CO. Calculate, per kilomole of mixture, the mass of mixture to be removed and the mass of CO to be added. The pressure and temperature in the vessel remain constant during the process. Take the molar mass of H2...
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 flask is filled with 4.0 atm of gaseous H2 and 3.0 atm of gaseous N2....
A flask is filled with 4.0 atm of gaseous H2 and 3.0 atm of gaseous N2. When a lit match is thrown into the flask, the gases react and form gaseous NH3. What is the pressure in the flask after the reaction? Answer: 4.33 atm. Please provide step by step on how to solve.
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
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT