Air is a mixture of gases with the following mass percentage composition: 75.52% N2, 23.15% O2, 1.28% Ar, and 0.046% CO2 (a) What are the partial pressures of N2, O2, Ar, and CO2, when the total pressure is 1.100 atm? (b) Calculate the molar Gibbs energy of mixing of air at 25 °C assuming ideal-gas behavior. (c) Determine the molar enthalpy of mixing and the molar entropy of mixing for air at 1.100 atm and 25 °C.
Air is a mixture of gases with the following mass percentage composition: 75.52% N2, 23.15% O2,...
The composition of air is approximately 75.52% N_2, 23.15% O_2, 1.28% Ar, and 0.046% CO_2. (a) Ignoring contributions from the other trace components of air, calculate the entropy of mixing of air when it is artificially prepared from its pure gas components. (b) At standard pressure, air liquefies at T = 78.8 K. At this temperature, the Ar and CO_2 have both frozen out of the air solution. The remaining liquid-phase air is stable between 58 K and 78.8 K....
5. a) The composition of a mixture of nitrogen and carbon dioxide gases is 30%-N, and 70%- CO2 by mole fraction. What is the mass fraction of the nitrogen constituent?b) Nitrogen (N2) at 150 kPa, 40°C occupies a closed, rigid container having a volume of 1 m3. If 2 kg of oxygen (O2) is added to the container, what is the molar analysis of the resulting mixture? If the temperature remains constant, what is the pressure of the mixture, in...
The mass percentage composition of dry air at sea level is approximately N2: 75.5; O2: 23.2; Argon: 1.3. What is the partial pressure of each component when the total pressure is 1.60 atm?
You have a mixture of the gases Cl2 and O2 along with some N2 in a container at STP. The moles of Cl2 and O2 in the mixture are equivalent and the density of the mixture is 1.951 g/L. Assuming ideal behavior, what is the mole fraction of N2 in the mixture?
The composition by mass of air is 79% N2, 20% O2, and 1% Ar. Calculate the density of O2 at 25°C and 750 torr. pressure.
This is physical chemistry problem from Atkins 5. [20 (1) The variation of chemical potential, u of a perfect gas with pressure can be expressed as follows: Au RT ln Derive the below equation for Gibbs energy of mixing, when two gases of A and B are mixed at constant pressure, p and temperature, T. (2) Calculate the molar Gibbs energy of mixing when the two major components of air (nitrogen and oxygen) are mixed to form air at 298...
A mixture of gases has the composition given in Table 1. It has a total mass of 3.46 kg, and has an initial volume and temperature of 1.273 m3 and 300 K respectively. The mixture undergoes polytropic compression to a final volume of 0.5 m3. The polytropic index for this process is known to be 1.2. Table 1: Volumetric analysis of a mixture of gases Constituent Gas Chemical Symbol Volumetric Analysis ViV Molar Mass m˜i [kg/kmol] Specific Heat Capacity at...
A mixture of He, Ar, and Xe has a total pressure of 2.80 atm . The partial pressure of He is 0.300 atm , and the partial pressure of Ar is 0.300 atm . What is the partial pressure of Xe? A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250 mole O2 , and an unknown quantity of He. The temperature of the mixture is 0 ∘C , and the total pressure is 1.00 atm...
A gas mixture contains each of the following gases at the indicated partial pressures: N2, 216 torr ; O2, 123 torr ; and He, 122 torr . What is the total pressure of the mixture? What mass of each gas is present in a 1.30 −L−L sample of this mixture at 25.0 ∘C∘C?
Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. a) If the total pressure of the gases is 0.985 atm, calculate the partial pressure of each component of the mixture. b) If the volume of the exhaled gas is 455mL and its temperature is 37 degrees Celcius , calculate the number of moles of CO2 exhaled. c) How many grams of glucose (C6H1206) would need to be metabolized to produce...