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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H2O(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 7.78 L, the number of moles of Al reacted was pressure of water is 23.8 mm Hg at 25 °C.
Please help me to give you thumbs up
Calculate the partial pressure of propane (C3H8) in a mixture that contains equal masses of propane and butane (C4H10) at 50°C and 764 Torr.
What pressure (in torr) of carbon dioxide gas can be produced by the combustion of 1.00 g of benzene (C6H6) in a closed, 25.0 L container at a temperature of 15°C? 2C6H6(l)+15O2(g)-->12CO2(g)+6H2O(l)
Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KC103 (8) 2KCl(s) + 302(g) The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 757.0 mm Hg. If the wet O₂ gas formed occupies a volume of 5.22 L, the number of moles of KCIO, reacted was 5.3 mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride, as shown in the reaction below. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) A) 4 × 10–3 L B) 2.2 L C) 2.9 L D) 5.8 L E) 11.7 L
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH, (g) +3 Cl, () 2CH,CI(g) + 2 HCI(g) + 2CI (g) Suppose that a chemist combines 273 mL of methane and 689 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 75.0% completion, what is the total pressure in the flask? Pictal = atm What is the partial pressure of CH,? Pon, = atm What is the partial pressure of Cl, ?
Consider the reaction shown below: 2 HCl (aq) + CaCO3 (s) ⟶ CO2 (g) + CaCl2 (aq) + H2O (l) How many grams of CaCO3 would need to be consumed to fill a 908.001 mL balloon with CO2 gas, assuming a constant temperature of 21.7 oC and constant pressure of 0.958 atm? Express your answer in units of grams using at least three significant figures.