An ideal gas mixture contains 35% helium, 20% methane, and 45% nitrogen by volume at 2.00 atm absolute and 90 C. Calculate: A. Draw an illustration of the problem/systematic diagram B. The partial pressures of each component C. The mass fraction of each component D. The average molecular weight of the gas E. The density for the gas in kg/m3 (Universal gas constant = 8.3143 kj/kg-k)

An ideal gas mixture contains 35% helium, 20% methane, and 45% nitrogen by volume at 2.00 atm absolute and 90 C. Calculate: A. Draw an illustration of the problem/systematic diagram B. The partial pressures of each component C. The mass fraction of each component D. The average molecular weight of the gas E. The density for the gas in kg/m3 (Universal gas constant = 8.3143 kj/kg-k)

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.32E

See similar textbooks

Similar questions

A fuel contains 78wt% carbon and 22wt% hydrogen (H). Combustion results in the following composition by volume (dry basis): CO2 : 9.41 CO : 1.69 O2 : 3.8 N2: 85.1 The following equations describe the chemical reactions taking place: CO+0.5 O2→ CO2 C+O2→ CO2 H2 + 0.5 O2 → H2O C+0.5O2→ CO On the basis of 120 lb moles of dry flue gas, the O2 required (lb moles) for complete combustion is most nearly. Find the amount of O2 needed for the completion of combustion
stack gas analysis: 83.08% N2, 7.5% CO2, 2.3% CO, 1.12% H2, 6% O2 with a saturation temperature of 54°C at 400°C and 760mmHg. a) %excess of air (1000 m^3 of air is supplied, produced 3100 m^3 of stack gas) b) chemical formula of the fuel burned c) analysis of the fuel mixture
c. A mixture of propane and methane occupied 122 mL at 25⁰C and 1.0 atm. This mixture was totally burned in excess O2 to produce CO2(g) and H2O(g). The mass of the CO2 produced was 0.506 g. What is the mass % composition of the original mixture? Show all work.
Ammonia (considered to be ideal gas, 1 mole) initially at 25 oC and 1 bar pressure is heated at constant pressure until the volume has tripled.Use CP = 25.895 + 32.999 x 10^– 3 T – 30.46 x 10^– 7 T2 , J/mole-KCalculate: c) delta H d) delta U e) delta S show complete solution
Gypsum (plaster of Paris : CaSO,. 2H,0) is produced by the reaction of calcium carbonate and sulfuric acid. A certain lime stone analyzes: CaCO, 96.89 %; MgCO, 1.41 %; inerts 1.70 %. For 5 metric tons of limestone reacted completely, determine: a. kg of anhydrous gypsum (CaSO,) produced. b. kg of sulfuric acid solution (98 wt%) required.
Calculate the partial pressure (Pa) of CO2 in a mixture that contains 45% wt CO2, 35% wt CO and 20% wt O2 at 100 deg C and 1.5 atm.
A gasification plant of MSW produces syngas of the following Component Composition (dry volume %) CO 30 H2 40 CO2 30 Determine the weight percentage of syngas component. (MW: CO =28; H2 = 2; CO2 = 44) (Hints: It is easier to start with 100 moles syngas and volume ratio is equal to molar ratio)
A fuel containing 75% ethane and 25% propane is burned with dry air. All the H2 burns to H2O and the CO2 to CO ratio is 11:1. 20% excess air is supplied. Calculate:a. Mole flue gas/100 moles of fuel b. Orsat analysis of the flue gas c. Complete analysis of the flue gas d. m3 dry air at 28 °C, 765 mmHg per kmol fuel
A flue gas contains 5 mole% H 2O. Calculate the ratios(a) kmol flue gas/kmol H 2O.(b) kmol dry flue gas/kmol flue gas.(c) kmol H 2 O/kmol dry flue gas.
The label has come off a cylinder of gas in your laboratory. You know only that one species of gas is contained in the cylinder, but you do not know whether it is hydrogen, oxygen, or nitrogen. To find out, you evacuate a 5-liter flask, seal it and weigh it, then let gas from the cylinder flow into it until the gauge pressure equals 1.00 atm. The flask is reweighed, and the mass of the added gas is found to be 13.0 g. Room temperature is 27°C, and barometric pressure is 1.00 atm. What is the gas?
To evaluate the use of renewable resources, an experiment was carried out with rice hulls. After pyrolysis, the product gas analyzed 6.4% CO2, 0.1% O2, 39% CO, 51.8% H2, 0.6% CH4, and 2.1% N2. It entered a combustion chamber at 90 °F and a pressure of 35.0 in. Hg and was burned with 40% excess air (dry) at 70 °F and an atmospheric pressure of 29.4 in. Hg; 10% of the CO remains. a. How many cubic feet of air were supplied per cubic foot of entering gas? b. How many cubic feet of product gas were produced per cubic foot of entering gas if the exit gas was at 29.4 in. Hg and 400 °F?
Show complete solutions and enclose all final answers in a box. Round off final answers to 4 decimal places and use floating values for intermediate answers. A gas column is separated into two segments by a non-permeable partition. On the first segment is 1.63 moles of Helium with volume V1 and on the second segment is 3.84 moles of Oxygen gas with volume V2. Consider both gases to be ideal and at the same pressure P and temperature T. If the partition is removed, calculate the change in entropy of the gaseous system.