3. 1.32 mmol of an ideal gas are expanded at the constant temperature of 298K. Calculate the Volume the gas will occupy at the pressures provided in the table below. Pressure (atm) Volume (L) density (g/L) (Ref. 5c) 1 0.5 0.1 0.05 0.01 0.005 b. Plot the data in a (x,y) = (V,P) set of Cartesian coordinates.
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- A N2 gas is pumped into a container with 39.6 L volume at 298.15 K and the final pressure reads 15.3 bar in the container. Then additional O2 gas is pumped in and the final total pressure reads 34.4 bar in the container. Estimate the molar fraction of O2 gas in the mixture. x_O2 = ______ 3 sig. figure. Suggest using Excel to organize data and calculate for this and the next two questions.A glass container was initially charged with 2.60 moles of a gas sample at 3.75 bar and 21.7 C. some of the gas was released as the temperature was increased to 28.5 C, so the final pressure in the container was reduced to 0.998 bar. how many moles of the gas sample are present at the end?A gas in a cubical container with side equal to 0.3568 m has a pressure of 0.24 MPa at 24°?. If the gas constant is equal to 212 j/(kg-K), Compute the following, a. Density of the gas in kg/m^3, b. Mass of the gas in lbm , c. Weight of the gas in N
- Calculate the pressure exerted in atm by 3.0 moles of ammonia when it is behaving as (a) a perfect gas in atm at 25°C in 22.414L and (b) van der Waals (VDW) gas at 100°C in 1000.0 cm3. Given van der Waals constants: a(NH3) (L2.atm/mol2) = 4.17 and b(NH3)(L/mol) = 0.037. Use 273.15 K for the temperature conversion. Pperfect gas = [A] atm PVDW = [B] atm 3 sig. figures normal format. Note: There is no need to add the units. The numerical values is sufficient as long as it is calculated in atm. Please also indicate the sign if it is necessary without a space from the numerical answer.The Dieterici equation of state is similar to the van der Waals equation in that they both employ gas-specific constants a and b to attempt to account for the interaction between molecules and the nonzero volume of the individual molecules of gas. However, the Dieterici equation of state has a significantly different functional form: ?(? − ?) = ??? -a ⁄ (RVT) Note that a and b are constants (n is implicitly constant as volume is expressed as molar volume). What are the following partial derivatives for the Diererici equation of state? a) (∂P/∂T)V b) (∂V/∂P)TCarbon monoxide and molecular oxygen react to form carbon dioxide. A 50.0 L reactor at 25.0 oC is charged with 1.00 bar of CO. The gas is then pressurized with O2 to give a total pressure of 3.50 bar. The reactor is sealed, heated to 350 oC to drive the reaction to completion, and cooled back to 25.0 oC. Compute the final partial pressure of each gas (in bar).
- What is the volume (m3) of 1 mol of a gas occupied at the standard temperature and pressure conditions [T = 0oC = 273 K and P = 1 atm = 1.01 × 105 Pascals (N/m)]. Hint: Use Ideal gas equation. Enter your numerical value (answer) in 3 significant figures. Do not enter units.You have diaphragm pump that generates a 6.30 L internal volume when the diaphragm flexes. It is currently operating at 98.2oC. What is the pressure in atmospheres in the pump with each cycle? Estimate that exactly 1 mole=22.4L of air to determine the number of moles of gas in the pump. Assume air is behaving as an ideal gas.P1A.6 The molar mass of a newly synthesized fluorocarbon was measured in a gas microbalance. is device consists of a glass bulb forming one end of a beam, the whole surrounded by a closed container. e beam is pivoted, and the balance point is attained by raising the pressure of gas in the container, so increasing the buoyancy of the enclosed bulb. In one experiment, the balance point was reached when the fluorocarbon pressure was 327.10Torr; for the same setting of the pivot, a balance was reached when CHF3 (M = 70.014 g mol−1) was introduced at 423.22 Torr. A repeat of the experiment with a di erent setting of the pivot required a pressure of 293.22 Torr of the uorocarbon and 427.22 Torr of the CHF3. What is the molar mass of the fluorocarbon? Suggest a molecular formula.
- A certain gas obeys the van der Waals equation with a= 0.50 m6 Pa mol-2. Its volume is found to be 5.00 x 10-4m3 mol-1 at 273 K and 3.0 MPa. From this information calcu late the van derWaals constant b. What is the compression factor for this gas at the prevailing temperature and pressure?Estimate the molar volume of CO2 at 500K and 100 atm by treating it as a van der Waals gas.The van der Waals coefficients for CO2 are as follows: a=3.610 atm dm6 mol-3 and b=4.29x10-2 dm3 mol-1.a) A certain sample of gas has a volume of 20.0 dm3 at 0oC and 1.0 atm. A plot of the experimental data of its volume against the celcius temperature, Ɵ, at constant pressure, gives a straight line of slope 0.074 dm3 /o From these data alone (without use of the perfect gas law) determine the absolute zero of temperature in degrees Celsius? b) Ballons are still used to deploy sensors that monitor meteorological phenomena. It is possible to investigate some of the technicalities of ballooning by using perfect gas law. Suppose your balloon has a radius of 3.0 m and that is spherical. What mass of H2 (in mol) is needed to inflate it to 1.0 atm in an ambient temperature of 25oC at sea level? What mass can the balloon lift at sea level,where the density of air is 1.22 kg /m3? What would be the payload if He were used instead of H2?