An important process for the production of acrylonitrile (C3H3N) is given by the following equation: 2C3H6(g) + 2NH3(g) + 302(g) - 2C3H3N(g) + 6H20(g) A 150.-L reactor is charged to the following partial pressures at 25°C: PC3H6 = 0.500 MPa PNH3 =5 0.800 MPa Poz = 1.500 MPa What mass of acrylonitrile can be produced from this mixture (MPa = 10 Pa)? 1.61 x 10 g C3H;N 1.61 x 10 g C3H3N 2.87 x 10 g C3H3N 1.00 x 10 g C3H3N OOO O

An important process for the production of acrylonitrile (C3H3N) is given by the following equation: 2C3H6(g) + 2NH3(g) + 302(g) - 2C3H3N(g) + 6H20(g) A 150.-L reactor is charged to the following partial pressures at 25°C: PC3H6 = 0.500 MPa PNH3 =5 0.800 MPa Poz = 1.500 MPa What mass of acrylonitrile can be produced from this mixture (MPa = 10 Pa)? 1.61 x 10 g C3H;N 1.61 x 10 g C3H3N 2.87 x 10 g C3H3N 1.00 x 10 g C3H3N OOO O

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter6: The States Of Matter

Section: Chapter Questions

Problem 6.43E

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61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
The barometric pressure measured outside an airplane at 9 km (30,000 ft) was 266 torr. Calculate the pressure in kPa.
In the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.
A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?

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